Answer:
K = 6.5 × 10⁻⁶
Explanation:
C₅H₆O₃(g) → C₂H₆(g) + 3 CO(g)
The formula for the ideal gas law
PV = nRT
where
P = total pressure
V = volume
n = total moles
R = gas constant
T = absolute temperature
P(C₅H₆O₃) = nRT/V
where
n = 5.63 /114
= 0.049
[tex]= \frac{0.049 * 0.0821 * 473}{2.5}[/tex]
= [tex]0.78atm[/tex]
C₅H₆O₃(g) ⇄ C₂H₆(g) + 3 CO(g)
0.78atm 0 0
0.78 - x x 3x
P(total) = 1.63atm
0.78atm - x + x + 3x⇒x = 0.288atm
P(C₅H₆O₃) = 0.78 - 0.288
= 0.489 atm
P(C₂H₆) = 0.288 atm
P(CO) = 0.846 atm
[tex]Kp = \frac{0.288 * 0.864^3}{0.489}[/tex]
= 0.379
K = Kp/(RT³)
[tex]= \frac{0.379}{(0.0821 * 473)^3} \\= 6.5 * 10^-^6[/tex]
K = 6.5 × 10⁻⁶
The value of K for this reaction is : 6.5 * 10⁻⁶
The decomposition equation
C₅H₆O₃ ----> C₂H₆ (g) + 3 CO (g)
Given data :
mass of pure C₅H₆O₃ = 5.63 g
volume of flask = 2.50 L
Temperature = 200°C = 473 K
Pressure in flask = 1.63 atm
Determine the value of K for this reactionwe will apply Ideal gas law formula
PV = nRT
therefore P( C₅H₆O₃ ) = nRT / V ---- ( 1 )
where : n = 5.63 / 114 = 0.049, V = 2.5 L, R = 0.0821, T = 473 k
Insert values into equation ( 1 )
P( C₅H₆O₃ ) = 0.78 atm - x ---- ( 2 )
P(total) = 1.63 atm.
Considering the decomposition equation
0.78 - x + x + 3x = 1.63 atm
therefore ; x = 0.288
back to equation ( 2 )
P( C₅H₆O₃ ) = 0.78 - 0.288 = 0.489 atm
Given that :
P(C₂H₆) = 0.288 atm
P(CO) = 0.846 atm
Find K using the relationship below
K = Kp / ( RT)³ ------ ( 3 )
While Kp = ( 0.288 * 0.864³ ) / 0.489
= 0.379
Back to equation ( 3 )
K = 0.379 / ( 0.0821 * 473 )³
= 6.5 × 10⁻⁶.
Hence we can conclude that the value of K for this reaction is : 6.5 * 10⁻⁶
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The pressure of a gas at the triple point of water is 1.20 atm. Part A If its volume remains unchanged, what will its pressure be at the temperature at which CO2CO2 solidifies?
The pressure P2 at the temperature which CO2 gets solidifies is 0.857 atm.
Explanation:
The relation between temperature T and the pressure P is that it is proportional to each other.
T ∝ P
As the temperature decreases, the pressure also decreases which is given by
T1 / T2 = P1 / P2
At the triple point of water, the temperature equals 273 K.
Consider T1 = 273 K, P1 = 1.20 atm
The temperature T2 of the CO2 solidifies equals 195 K
(273 / 195) = (1.20 / P2)
P2 = (195 x 1.20) / 273
P2 = 0.857 atm.
The pressure P2 at the temperature which CO2 gets solidifies is 0.857 atm.
Select the compound that is most likely to increase the solubility of ZnSe when added to water.NaCnMgBr2NaClKClO4
Final answer:
NaCN is likely to increase the solubility of ZnSe in water due to complexation with Zn2+, which drives the dissolution equilibrium forward.
Explanation:
The question asks which compound is most likely to increase the solubility of ZnSe when added to water. Considering the principles of solubility and the common ion effect, the best compound to increase ZnSe solubility would not be one that provides a common ion, as that would decrease solubility. Among the options provided, NaCN seems to be the most suitable choice.
Cyanide ions from NaCN can form a complex with Zn2+, effectively removing Zn2+ from the solution and driving the dissolution equilibrium of ZnSe forward. This complexation increases the solubility of ZnSe due to Le Chatelier's principle, where the reaction shifts to alleviate the stress of the added CN- ions by dissolving more ZnSe.
Suppose that the uncertainty in determining the position of an electron circling an atom in an orbit is 0.4 A. What is the uncertainty in its velocity
Answer:
Explanation:
Applying the Heisenberg uncertainty principle,
Δx X mΔv = h/4π
where Δx = uncertainty in measurement of position
Δv = uncertainty in measurement of velocity
m = mass of object
h = planck's constant
Here:
Δv = 0.4 A° = 4.0 x 10^-11 m
mass, m = 9.11 x 10^-31 Kg
Plugging the values,
4.0 x 10^-11 x Δ v = (6.626 x 10^-34) / (4 x 3.14 x 9.11E-31)
4.0 x 10^-11 x Δ v = 5.791 x 10^-5
Δv = 1.448 x 10^6 m/s, the uncertainty in its velocity
Answer = 1.45 x 10^6 m/s
The uncertainty in an electron's velocity, given an uncertainty in its position, is calculated using the Heisenberg Uncertainty Principle. By applying the principle's formula with the given position uncertainty and known electron mass, we can determine the minimum uncertainty in the electron's velocity.
Explanation:The question pertains to the Heisenberg Uncertainty Principle which is a fundamental concept in quantum physics that describes the limit to the precision with which certain pairs of physical properties of a particle, such as position and momentum, can be known simultaneously. To find the uncertainty in velocity, we use the principle's formula ΔxΔp >= ĩ/2, where Δx is the uncertainty in position, Δp is the uncertainty in momentum, and ĩ is the reduced Planck's constant (about 1.055 × 10-34 Js). Since momentum is mass times velocity (p = mv), the uncertainty in velocity (Δ4v) can be found by rearranging the formula to Δ4v >= (ĩ/(2mΔ4x)).
Given that the uncertainty in the position (Δ4x) is 0.4 Å, which is 0.4 × 10-10 meters, and assuming the electron's mass (m) as 9.11 × 10-31 kg, we can calculate the minimum uncertainty in the electron's velocity using the formula.
Remember, this is a simplification and in real-world applications, one would need to account for other factors that could affect the measurement.
Consider mixture C, which will cause the net reaction to proceed in reverse. Concentration (M)initial:change:equilibrium:[XY]0.200+x0.200+x←net⇌[X]0.300−x0.300−x+[Y]0.300−x0.300−x The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed.
This is an incomplete question, here is a complete question.
Calculating equilibrium concentrations when the net reaction proceeds in reverse Consider mixture C, which will cause the net reaction to proceed in reverse.
The chemical reaction is:
[tex]XY(g)\rightleftharpoons X(g)+Y(g)[/tex]
Concentration(M) [XY] [X] [Y]
(M)initial: 0.200 0.300 0.300
change: +x -x -x
equilibrium: 0.200+x 0.300-x 0.300-x
The change in concentration, x, is positive for the reactants because they are produced and negative for the products because they are consumed. Based on a Kc value of 0.140 and the data table given, what are the equilibrium concentrations of XY, X, and Y, respectively?
Answer : The Equilibrium concentrations of XY, X, and Y is, 0.104 M, 0.204 M and 0.204 M respectively.
Explanation :
The chemical reaction is:
[tex]XY(g)\rightleftharpoons X(g)+Y(g)[/tex]
initial: 0.200 0.300 0.300
change: +x -x -x
equilibrium: (0.200+x) (0.300-x) (0.300-x)
The equilibrium constant expression will be:
[tex]K_c=\farc{[X][Y]}{[XY]}[/tex]
Now put all the given values in this expression, we get:
[tex]0.140=\frac{(0.300-x)\times (0.300-x)}{(0.200+x)}[/tex]
By solving the term 'x', we get:
x = 0.0963 and x = 0.644
We are neglecting the value of x = 0.644 because the equilibrium concentration can not be more than initial concentration.
Thus, the value of x = 0.0963
Equilibrium concentrations of XY = 0.200+x = 0.200+0.0963 = 0.104 M
Equilibrium concentrations of X = 0.300-x = 0.300-0.0963 = 0.204 M
Equilibrium concentrations of X = 0.300-x = 0.300-0.0963 = 0.204 M
In the context of equilibrium chemistry, a net reaction can proceed in either direction until equilibrium is reached. In this case, mixture C causes the reaction to shift in the reverse direction, thereby increasing the concentration of the reactants and decreasing the concentration of the products. This continues until the forward and reverse reaction rates equalize, achieving a state of equilibrium.
Explanation:The process being described in your question is related to chemical equilibrium. When we speak about a reaction reaching equilibrium, it describes the point at which the concentrations of reactants and products do not change over time. This doesn't mean the reaction has stopped, but instead, the forward and reverse reactions are happening at the same rate due to the dynamic nature of chemical equilibria. In the case of your query, mixture C will cause the net reaction to proceed in reverse.
Using your example, [XY] represents the reactant and [X] and [Y] represent the products. Since the reaction shifts in the reverse direction, the reactants (the products in the forward reaction) increase, hence the positive change in concentration, 'x'. This process continues until the forward and reverse reaction rates become equal, which signifies the reaction's equilibrium state where concentrations of its reactants and products remain constant.
The aforementioned process is guided by the principle of Le Chatelier's, which states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
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Consider the following generic chemical equation: A + B → C + D Reactant A contains 85.1 J of chemical energy. Reactant B contains 87.9 J of chemical energy. Product C contains 38.7 J of chemical energy. If the reaction absorbs 104.3 J of chemical energy as it proceeds, how much chemical energy must product D contain
Answer:
= 238.6J
Explanation:
According to the law of conservation of energy, energy can neither be created nor be destroyed. It can only be transformed from one form to another.
Endothermic reactions are those in which heat is absorbed by the system and thus the energy of products is higher than the energy of reactants.
For the given reaction:
A + B ⇄ C + D
Energy of A = 85.1 J
Energy of B = 87.9 J
Product C contains 38.7 J
Energy balance:
∑ enthalpy of the reactants + energy added = ∑ enthalpy of the products + energy released.
∑ enthalpy of the reactants = 85.1 J + 87.9 J = 173 J
energy added = 104.3 J
∑ enthalpy of the products = 38.7 J + D
energy released = 0
Equation:
173J + 104.3J = 38.7 + D + 0
⇒ D = 173J + 104.3J - 38.7J
= 238.6J
which is the chemical energy of the product D
Product D must contain 238.6 J of chemical energy based on the principles of energy conservation in a chemical reaction.
In a chemical reaction, the law of conservation of energy states that energy cannot be created or destroyed; it can only change forms. This principle applies to chemical energy as well. Therefore, the total energy in the reactants must equal the total energy in the products.
Let's analyze the given information and calculate the chemical energy in product D:
Reactant A contains 85.1 J of chemical energy.
Reactant B contains 87.9 J of chemical energy.
Product C contains 38.7 J of chemical energy.
The total initial chemical energy in the reactants (A and B) is:
Initial Energy (A + B) = 85.1 J + 87.9 J = 173.0 J
The reaction absorbs 104.3 J of chemical energy as it proceeds. This means that the total energy in the products (C + D) must be equal to the initial energy plus the absorbed energy:
Total Energy in Products (C + D) = Initial Energy (A + B) + Absorbed Energy
Total Energy in Products (C + D) = 173.0 J + 104.3 J = 277.3 J
Now, we know the total energy in the products (C + D) is 277.3 J, and we already know the energy in product C is 38.7 J. To find the energy in product D, we can subtract the energy in C from the total energy in the products:
Energy in Product D = Total Energy in Products - Energy in Product C
Energy in Product D = 277.3 J - 38.7 J = 238.6 J
Therefore, product D must contain 238.6 J of chemical energy.
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The molar enthalpy of vaporization (∆Hvap) for ammonia (NH3) is 23.3 kJ/mol (at −33.3 °C). How much energy is required to evaporate 100. g of ammonia at this temperature?
Answer: 137 kJ
Explanation:
Latent heat of vaporization is the amount of heat required to convert 1 mole of liquid to gas at atmospheric pressure.
To calculate the moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{100g}{17g/mol}=5.9moles[/tex]
1 mole of ammonia requires heat = 23.3 kJ
Thus 5.9 moles of ammonia require heat =[tex]\frac{23.3}{1}\times 5.9=137kJ [/tex]
Thus the energy is required to evaporate 100 g of ammonia at this temperature is 137 kJ
Final answer:
To evaporate 100 g of ammonia at -33.3 °C, 136.76 kJ of energy is required.
Explanation:
To calculate the amount of energy required to evaporate 100 g of ammonia at -33.3 °C, we need to use the molar enthalpy of vaporization (∆Hvap). The ∆Hvap for ammonia is 23.3 kJ/mol. First, we need to convert the mass of ammonia to moles using its molar mass. The molar mass of ammonia is 17.03 g/mol. So, 100 g of ammonia is equal to 100/17.03 = 5.87 mol. Now, we can calculate the energy required:
Energy required = ∆Hvap × number of moles = 23.3 kJ/mol × 5.87 mol = 136.76 kJ
a 25% alcohol solution is to be mixed with a 40% alcohol solution to obtain 18 liters of a 30% alcohol solution. How many liters of each solution should be used
Answer : The volume of solution used should be, 12 L
Explanation :
Let the volume of solution be, x
Thus the equation will be:
[tex]25\%\times (x)+40\%\times (18-x)=30\%\times (18)[/tex]
Now solving the term 'x', we get:
[tex]\frac{25}{100}\times (x)+\frac{40}{100}\times (18-x)=\frac{30}{100}\times (18)[/tex]
[tex]0.25\times (x)+0.4\times (18-x)=0.3\times (18)[/tex]
[tex]0.25x+7.2-0.4x=5.4[/tex]
[tex]-0.15x=-1.8[/tex]
[tex]0.15x=1.8[/tex]
[tex]x=12[/tex]
Thus, the volume of solution used should be, 12 L
If it takes 43.32ml of .1M NaOH to neutralize a 50ml HCL solution, how many moles of NaOH were added to the HCL solution?
Answer:
4.332 millimoles of NaOH
Explanation:
Molarity (M) = moles per liter (mole/L); liters x moles/liter = moles
0.04332 L x 0.1 mole/liter = 0.004332 moles of NaOH (4.332 millimoles)
millimoles / milliliters = moles/liter = molarity (M).
4.332 millimoles / 50 milliliters = 0.08664 M HCl
In the Volumetric titration at the end point, moles of NaOH = moles of HCl
NaOH + HCl --> H2O + NaCl
When a solution of AgNO3 is mixed with a solution of NaBr (multiple options could be correct):
1) NaNO3 precipitate will spontaneously form.
2) After a few minutes pass, the concentration of Ag+ and Br- will be lower than when the two solutions were first mixed.
3) After a few minutes pass, the concentration of Ag+ and Br- will be the same as when the two solutions were first mixed
4) The concentration of Ag+ and Br- are momentarily greater than in a saturated solution of AgBr.
5) AgBr precipitate will spontaneously form.
Answer:
After a few minutes pass, the concentration of Ag+ and Br- will be lower than when the two solutions were first mixed.
AgBr precipitate will spontaneously form.
Explanation:
After the net ionic equation AgBr forms
The reaction between AgNO3 and NaBr leads to the formation of AgBr, a precipitate, and NaNO3, which remains dissolved in the solution. The concentration of Ag+ and Br- ions in the resulting solution will therefore be decreased.
Explanation:When a solution of AgNO3 is mixed with a solution of NaBr, a double displacement reaction or metathesis occurs, producing AgBr and NaNO3. According to solubility rules, AgBr is a precipitate, hence the options 2 and 5 are correct: After a few minutes, the concentration of Ag+ and Br- ions will be lower than when the two solutions were first mixed, and AgBr precipitate will spontaneously form. On the other hand, NaNO3 is soluble in water, so it remains dissolved and no precipitate of NaNO3 forms, which makes option 1 incorrect. Options 3 and 4 are also incorrect because the concentration of Ag+ and Br- ions will decrease as they form a precipitate and won't exceed the saturation point of AgBr.
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When you add "plant food" to your potted geraniums, you are actually providing the plant with _____. View Available Hint(s) When you add "plant food" to your potted geraniums, you are actually providing the plant with _____. complex carbohydrates vitamins and amino acids sugars minerals
Answer:
minerals
Explanation:
A potted geranium is plant that is capable of manufacturing complex carbohydrates from sugar synthesized through the process of photosynthesis.
The process of photosynthesis primarily requires water and carbohydrate together with resources such as essential minerals. Hence, when a plant food is added to a plant, the most plausible term this refers to is minerals. This is because food contains minerals necessary for various metabolic activities of living organisms.
What is the central atom of C2H4Br2
Answer:
1.2,dibromoethane is the sha'awa .
The central atom in C2H4Br2 is a carbon (C) atom, with each carbon atom being central to its respective part of the molecule, exhibiting a trigonal planar shape and bond angles of approximately 120°.
Explanation:The central atom in C2H4Br2 is a C (carbon) atom, with other C, H (hydrogen), and Br (bromine) atoms as surrounding atoms. In this molecule, there are typically two central C atoms which are connected by a double bond, and each C atom has attached hydrogen and bromine atoms. Commonly in molecules, the central atom is the least electronegative element that is not hydrogen or a halogen, as these are usually terminal atoms. In C2H4Br2, each carbon atom is the central atom of its respective part of the molecule, with a trigonal planar shape due to the double bond and the single bonds to hydrogen and bromine. This arrangement leads to bond angles of about 120° around each central C atom.
Consider the reaction for the decomposition of hydrogen disulfide: 2H2S(g)⇌2H2(g)+S2(g), Kc = 1.67×10−7 at 800∘C A 0.500 L reaction vessel initially contains 0.163 mol of H2S and 5.00×10−2 mol of H2 at 800∘C. Find the equilibrium concentration of [S2].
Final answer:
The equilibrium concentration of [[tex]S_2[/tex]] is [tex]1.12 \times 10^{-3} M[/tex].
Explanation:
To find the equilibrium concentration of [[tex]S_2[/tex]], we need to use the equilibrium constant expression [tex]\( K_c = \frac{{[H_2]^2[S_2]}}{{[H_2S]^2}} \)[/tex]. Given the initial concentrations of [tex]H_{2}S[/tex] and [tex]H_2[/tex], and assuming x moles of [tex]H_{2}S[/tex] decompose, we can set up an ICE table and solve for the equilibrium concentrations. Substituting the equilibrium concentrations into the equilibrium constant expression and solving for [[tex]S_{2[/tex]], we find the equilibrium concentration to be [tex]1.12 \times 10^{-3} M[/tex]. This indicates the concentration of [tex]S_2[/tex] at equilibrium after the reaction has reached its dynamic equilibrium state at 800°C.
The compound responsible for the characteristic smell of garlic is allicin, The mass of 1.00 mol of allicin, rounded to the nearest integer, is __________ g.
Answer:
The mass of 1.00 mol of allicin, rounded to the nearest integer, is 162 g
Explanation:
Allicin is a compound that derivates from the alliin which is produced by the catalyzis of an enzime.
The molecular formula is: C₆H₁₀OS₂.
Let's determine the molar mass which is the mass that corresponds to 1 mol
Molar mass C . 6 + Molar mass H . 10 + Molar mass O + Molar mass S . 2 =
12 g/mol . 6 + 1 g/mol . 10 + 16 g/mol + 32.06 g/mol . 2 = 162.1 g/mol
The mass of 1 mole of allicin has been 162 g.
Allicin has been the organic compound of carbon, hydrogen, and sulfur. It has a molecular formula, [tex]\rm C_6H_10OS_2[/tex].
For the calculation of mass in a mole compound, the molecular mass of the compound has been given as:
[tex]mwt=M_C\;+\;M_H\;+\;M_O\;+\;M_S[/tex]
Where the mass of carbon, [tex]M_C=12\;\rm g/mol[/tex]
The mass of hydrogen, [tex]M_H=1\;\rm g/mol[/tex]
The mass of oxygen, [tex]M_O=16\;\rm g/mol[/tex]
The mass of sulfur, [tex]M_S=32\;\rm g/mol[/tex]
Substituting the values for molar mass of allicin as:
[tex]mwt=(6\;\times\;12)\;+\;(10\;\times\;1)\;+\;(1\;\times\;16)\;+\;(2\;\times\;32)\\mwt=72\;+\;10\;+\;16\;+\;64\;\text{g/mol}\\mwt=162\;\text{g/mol}[/tex]
The molar mass of allicin has been 162 g/mol.
The mass of 1 mole sample has been given as:
[tex]\rm Mass=moles\;\times\;\textit {mwt}[/tex]
Substituting the values for the mass of allicin as:
[tex]\rm Mass=1\;mol\;\times\;162\;g/mol\\Mass=162\;g[/tex]
The mass of 1 mole of allicin has been 162 g.
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Let us write the appropriate equilibria and associate the correction [tex]K_b[/tex] values. Remember, we will want to calculate the concentrations of all species in a 0.390 M Na ₂SO₃ (sodium sulfite) solution. The ionization constants for sulfurous acid are [tex]K_a_1[/tex] = 1.4 × 10⁻² and [tex]K_a_2[/tex] = 6.3 × 10⁻⁸.
Explanation:
The relation between [tex]K_a\&K_b[/tex] is given by :
[tex]K_w=K_a\times K_b[/tex]
Where :
[tex]K_w=1\times 10^{-14}[/tex] = Ionic prodcut of water
The value of the first ionization constant of sodium sulfite = [tex]K_{a1}=1.4\times 10^{-2}[/tex]
The value of [tex]K_{b1}[/tex]:
[tex]1\times 10^{-14}=1.4\times 10^{-2}\times K_{b1}[/tex]
[tex]K_{b1}=\frac{1\times 10^{-14}}{1.4\times 10^{-2}}=7.1\times 10^{-13}[/tex]
The value of the second ionization constant of sodium sulfite = [tex]K_{a2}=6.3\times 10^{-8}[/tex]
The value of [tex]K_{b2}[/tex]:
[tex]1\times 10^{-14}=6.3\times 10^{-8}\times K_{b1}[/tex]
[tex]K_{b1}=\frac{1\times 10^{-14}}{6.3\times 10^{-8}}=1.6\times 10^{-7}[/tex]
Final answer:
To find the equilibrium constant for the ionization of HSO4−, we use the equilibrium concentrations of H3O+, HSO4−, and SO42− in the given reaction formula to compute Ka.
Explanation:
To compute the equilibrium constant for the ionization of the HSO4− ion, we need to use the expression for the equilibrium constant (Ka) which is based on the concentrations of products over reactants, excluding water because its concentration is considered constant in dilute aqueous solutions. The given equilibrium is HSO4−(aq) + H2O(l) ⇒ H3O+(aq) + SO42−(aq). Given equilibrium concentrations are [H3O+] = 0.027 M, [HSO4−] = 0.29 M, and [SO42−] = 0.13 M. Hence, the equilibrium constant (Ka) is calculated as Ka = [H3O+][SO42-−]/[HSO4−] = (0.027)(0.13)/(0.29).
Ca3(PO4)2 + 3 H2SO4 ⟶ 2 H3PO4 + 3 CaSO4
Joaquin needs to react [m] grams of calcium phosphate. He will need to measure out ____ grams H2SO4 for this reaction.
Answer:
The answer to your question is below
Explanation:
Balanced chemical reaction
Ca₃(PO₄)₂ + 3H₂SO₄ ⇒ 2H₃SO₄ + 3CaSO₄
To answer this question just calculate the molar mass of both reactants.
Molar mass of Ca₃(PO₄)₂ = (3 x 40) + (2 x 31) + (8 x 16)
= 120 + 62 + 128
= 310 g
Molar mass of 3H₂SO₄ = 3[(2 x 1) + (1 x 32) + (4 x 16)]
= 3[2 + 32 + 64]
= 3[98]
= 294 g
Conclusion
310 g of Ca₃(PO₄)₂ will react with 294 g of 3H₂SO₄
When solid (NH4)(NH2CO2)(NH4)(NH2CO2) is introduced into an evacuated flask at 25 ∘C∘C, the total pressure of gas at equilibrium is 0.116 atmatm. What is the value of KpKp at 25 ∘C∘C?
Answer:
the value of Kp at 25°C is 2.37 × 10⁻⁴atm³
Explanation:
Given that Kp = 0.116atm
NH₄(NH₂CO₂)(s) ⇄ 2NH₃(g) + CO₂(g)
2x atm xatm
Pt = PNH₃ PCO₂
0.116 = 2x + x
0.116 = 3x
x = 0.116/3
x = 0.039 atm
PNH₃ = 2x =2(0.039) = 0.078 atm
PCO₂ = x = 0.039 atm
Now,
KP = PNH₃² × PCO₂
= 0.078² × 0.039 atm³
= 2.37 × 10⁻⁴ atm³
the value of Kp at 25°C is 2.37 × 10⁻⁴atm³
2' A mixture containing 2.75 gof ammonium chloride (NH4cl) in 5.0 g of water was heated to dissolve the solid and then allowed to cool in air. At 6f"C, the first crystals appeared in solution. What is the solubility of ammonium chloride (in g of NH4CIper 100 gof water) at 61 'C
Answer:
55g NH₄Cl / 100g Water
Explanation:
Solubility of a substance define the amount of solute per solvent in a saturated solution. The solution can dissolve additional solute if heated.
In the problem, as the first crystal appears at 61°C the solubility in this temperature is the concentration of the solution, that is:
2,75g NH₄Cl / 5,0g water ₓ 100 = 55g NH₄Cl / 100g Water
I hope it helps!
The solubility of ammonium chloride at 61°C is 55 grams per 100 grams of water.
The solubility of ammonium chloride at 61°C is 2.75 grams per 5 grams of water, which can be expressed as a ratio to find the solubility per 100 grams of water.
To find the solubility per 100 grams of water, we can set up a proportion:
[tex]\[\frac{2.75 \text{ g NH}_4\text{Cl}}{5 \text{ g water}} = \frac{x \text{ g NH}_4\text{Cl}}{100 \text{ g water}}\][/tex]
Now, we solve for [tex]\(x\)[/tex]:
[tex]\[x = \frac{2.75 \text{ g NH}_4\text{Cl}}{5 \text{ g water}} \times 100 \text{ g water}\] \[x = \frac{2.75}{5} \times 100\] \[x = 0.55 \times 100\] \[x = 55\][/tex]
The answer is: 55.
Write balanced chemical equations for the complete neutralization reactions that take place when the following acids are titrated with sodium hydroxide (a) hydrochloric acid, (b) acetic acid, and (c) phosphoric acid.
Answer:
(a) [tex]NaOH_{(aq)} + HCl_{(aq)} --> NaCl_{(aq)} + H_2O_{(l)}[/tex]
(b) [tex]NaOH_{(aq)} + CH_3COOH_{(aq)} --> CH_3COONa_{(aq)} + H_2O_{(l)}[/tex]
(c) [tex]H_3PO_4_{(aq)} + 3NaOH_{(aq)} --> 3H_2O{(l)} + Na_3PO_4_{(aq)}[/tex]
Explanation:
For a reaction involving sodium hydroxide and hydrochloric acid, the balanced equation of reaction is:
[tex]NaOH_{(aq)} + HCl_{(aq)} --> NaCl_{(aq)} + H_2O_{(l)}[/tex]
For a reaction involving sodium hydroxide and acetic acid, the balanced equation of reaction is:
[tex]NaOH_{(aq)} + CH_3COOH_{(aq)} --> CH_3COONa_{(aq)} + H_2O_{(l)}[/tex]
For a reaction involving sodium hydroxide and phosphoric acid, the balanced equation of reaction is:
[tex]H_3PO_4_{(aq)} + 3NaOH_{(aq)} --> 3H_2O{(l)} + Na_3PO_4_{(aq)}[/tex]
Final answer:
This answer provides balanced chemical equations for the neutralization reactions of hydrochloric acid, acetic acid, and phosphoric acid with sodium hydroxide.
Explanation:
Neutralization Reactions:
Hydrochloric Acid with Sodium Hydroxide: HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
Acetic Acid with Sodium Hydroxide: HC2H3O2(aq) + NaOH(aq) → NaC2H3O2(aq) + H₂O(l)
Phosphoric Acid with Sodium Hydroxide: H3PO4(aq) + 3NaOH(aq) → Na3PO4(aq) + 3H₂O(l)
The requirements for one type of atom to substitute for another in a solid solution are:_______.A. All substitutions must be limited to the same element. B. An atom must be identical in size. C. An atom must be similar in size. D. The substituting atom must be from the same period. E. The substituting atom must be from the same group.
Answer:
E. The substituting atom must be from the same group.
Explanation:
Usually members higher-up in the group can replace or substitute lower members of a group
A 10.0 mL 10.0 mL aliquot is removed from the described stock solution and diluted to a total volume of 100.0 mL. 100.0 mL. Calculate the molarity of the dilute solution.
The molarity of the dilute solution is 0.5 M.
The given parameters;
initial volume of the liquid, V₁ = 10 mLvolume of the diluted solution, V₂ = 100 mLConcentration of the initial stock, C = 5 MThe molarity of the dilute solution is calculated as follows;
[tex]C_{stock} = D.F \times c_{dilute}[/tex]
where;
D.F is dilute factor
The dilute factor of the given solution is calculated as follows;
[tex]D.F = \frac{V_{dilute}}{V_{concentrate}} \\\\D.F = \frac{100}{10} \\\\D.F = 10[/tex]
[tex]C_{stock} = D.F \times c_{dilute}[/tex]
[tex]5 = D.F \times c_{dilute}\\\\c_{dilute} = \frac{5}{DF} \\\\c_{dilute} = \frac{5}{10} \\\\c_{dilute} = 0.5 \ M[/tex]
Thus, the molarity of the dilute solution is 0.5 M.
"Your question is incomplete, it seems to be missing the following information":
A 10.0 mL of a liquid is removed from the described stock solution with molarity of 5M and diluted to a total volume of 100.0 mL. Calculate the molarity of the dilute solution.
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Alkanes and alkenes differ in that alkene molecules contain at least one:
A. oxygen atom
B. double bond
C. triple bond
D. chlorine atom
Answer:
Double bond
Explanation:
an alkene is a unsaturated hydrocarbon which means that it contain at least one double bond
Answer:
The answer to your question is B. double bond.
Explanation:
Both alkanes and alkenes are hydrocarbons composed by carbon and hydrogen.
The different between these compounds is that alkanes have only single bonds are are represented as: H H
| |
H - C - C - H
| |
H H
Alkenes have at least one double bound in their structure and are represented as
H - C = C - H
| |
H H
When a strong acid is titrated with a strong base using pheolphthalein as an indicator, the color changes abruptly at the endpoint of the titration and can be switched back and forth by the addition of only one drop of acid or base. The reason for the abruptness of this color change is that:
Final answer:
The abrupt color change in a titration using phenolphthalein occurs because this indicator exhibits a sharp transition at the equivalence point, which corresponds to a steep pH change when titrating strong acids with strong bases.
Explanation:
The abrupt color change observed when titrating a strong acid with a strong base using phenolphthalein as an indicator is due to the steep pH change that occurs at the equivalence point during the titration.
Phenolphthalein is a visual indicator that exhibits a clear and distinct color change—it turns from colorless to pink—around the equivalence point.
This sharp transition is suitable for accurately determining the end point of a titration between strong acids and bases, where the pH rises rapidly, allowing for the indicator to shift from its acidic form (colorless) to its basic form (pink) in a small volume interval of titrant addition.
The general chemistry of indicators can be represented by the equation: HIn(aq) → H+ (aq) + In¯¯(aq), where 'HIn' is the acid form of the indicator that is different in color compared to its ionized form 'In¯¯'.
Such distinct color changes of acid-base indicators are critical in titrations, since they provide a visual cue for the completion of the reaction without the need to continuously monitor the pH level.
A recent study has revealed that chlorinated hydrocarbons, gasoline and other volatile organic compounds (VOC's) have become significant pollutants in ________ from ________.
Answer:
ground water / leaking storage tanks
gas mixture with a total pressure of 765 mmHg contains each of the following gases at the indicated partial pressures: 131 mmHg CO2, 226 mmHg Ar, and 186 mmHg O2. The mixture also contains helium gas. what is the partial pressure of the helium gas
Answer:
322mmHg
Explanation:
To calculate the partial pressure of the helium gas, we use the Dalton’s law of partial pressure.
It states that for a mixture of gases which do not react, the total pressure is equal to the sum of the individual partial pressures.
This means that:
Total pressure = Partial pressure of CO2 + partial pressure of Ar + Partial pressure of O2 + Partial pressure of helium.
Hence, Partial pressure of the helium gas = 765-131-226-86 = 322 mmHg
Rank the solutions in order of decreasing [H3O ]. Rank solutions from largest to smallest hydronium ion concentration. To rank items as equivalent, overlap them. a. 0.10 M HNO3.
b. 0.10 M HCN.
c. 0.10 M HNO2.
d. 0.10 M HClO.e. smallest concentration.f. largest concentration.
Answer:
0.10M HCN < 0.10 M HClO < 0.10 M HNO₂ < 0.10 M HNO₃
Explanation:
We are comparing acids with the same concentration. So what we have to do first is to determine if we have any strong acid and for the rest ( weak acids ) compare them by their Ka´s ( look for them in reference tables ) since we know the larger the Ka, the more Hydronium concentration will be in these solutions at the same concentration.
HNO₃ is a strong acid and will have the largest hydronium concentration.
HCN Ka = 6.2 x 10⁻¹⁰
HNO₂ Ka = 4.0 x 10⁻⁴
HClO Ka = 3.0 x 10⁻⁸
The ranking from smallest to largest hydronium concentration will then be:
0.10M HCN < 0.10 M HClO < 0.10 M HNO₂ < 0.10 M HNO₃
Acids are substances that produce hydronium ions in solution.
According to Arrhenius definition, acids are substances that produce hydronium ions in solution. The concentration of these hydronium ions depends on the strength of the H-X bond.
The ease with which the H-X bond is broken to yield the proton is given by the Ka. The Ka is called the acid dissociation constant and shows the degree of ionization of an acid.
A strong acid has a high Ka hence it is completely dissociated in solution. A weak acid has a low Ka hence it dissociates only to a small extent in solution.
Given the equimolar solutions listed in the question, the order of hydronium ion concentration from smallest to largest is; HCN < HClO < HNO2< HNO3.
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A compound is composed of 13% carbon, 4.3% hydrogen, 30.4% nitrogen, and 52.2% oxygen. The mystery compound has a molar mass of 184 grams per mole. What is the molecular formula of the compound
Answer:
C₂H₈N₄O₆ is the molecular formula for the compound
Explanation:
Data from the problem:
13 g of C in 100 g of compound
4.3 g of H in 100 g of compound
30.4 g of N in 100 g of compound
52.2 g of O in 100 g of compound
Firstly we determine, the mass of each in 184 g of compound, which is 1 mol
(13 g / 100 g) . 184 g = 24 g C
(4.3 g / 100 g) . 184 g = 7.91 g H ≅ 8 g H
(30.4 g / 100 g) . 184 g = 56 g N
(52.2 g / 100 g) . 184 g = 96 g O
And now, we divide the mass by the molar mass of each to determine the moles:
24 g C / 12 g/mol = 2 mol C
8g H / 1 g/mol = 8 mol H
56 g N / 14 g/mol = 4 mol N
96 g O / 16 g/mol = 6 mol O
So the molecular formula of the compound is C₂H₈N₄O₆
Final answer:
To determine the molecular formula of the given compound, one must calculate the moles of each element from their percentages, derive the empirical formula, and scale it by the compound's molar mass. However, the provided data seems contradictory and does not accurately represent a real calculation process.
Explanation:
To determine the molecular formula of a compound with 13% carbon, 4.3% hydrogen, 30.4% nitrogen, and 52.2% oxygen with a molar mass of 184 grams per mole, we need to first calculate the empirical formula from the given percentages. Assuming we have 100 grams of this compound, the masses of each element would directly convert to grams (e.g. 13g C, 4.3g H, 30.4g N, and 52.2g O).
To find the moles of each element, we divide the mass of each by its atomic mass (C: 12.01, H: 1.01, N: 14.01, O: 16.00) and get the ratios of moles of each element. However, the provided dissolution involves an inaccurate representation of the compound's composition and seems to contradict the given percentages.
For an accurate molecular formula determination, we use the correct composition to find the lowest whole number ratio of elements and scale it up using the compound's molar mass. This approach accurately identifies the compound's molecular makeup by aligning the empirical formula mass to the given molar mass.
Given that ammonia is a gas at room temperature, what can you infer about the relative strengths of the intermolecular forces between ammonia molecules and between water molecules
Answer:
The answer to the question is;
The inter-molecular forces of water are stronger than those of hydrogen.
Explanation:
Ammonia is a compressible gas at room temperature with molecules free to move about and so fill up the volume of the container in which it is placed due to the weaker inter-molecular Van der Waals forces such as Keesom, Debye and London dispersion forces holding the particles of ammonia together in a given volume of the compound.
The inter-molecular forces between water molecules is hydrogen binding and dipole moments due to the strongly electronegative oxygen and hydrogen which tends to move the electrons towards the oxygen creating a charge imbalance that causes the hydrogen surrounding the water molecule to aggregate to neutralize the the charge imbalance forming the bases for the strong hydrogen bonds.
Therefore water is a liquid at room temperature while ammonia is a gas due to the difference in strength of their inter-molecular forces.
The intermolecular forces in water are stronger than the intermolecular forces in ammonia.
The intermolecular forces hold substances together in a particular state of matter. There are three states of matter;
SolidLiquid GasThe strongest degree of intermolecular interaction occurs between matter in the solid state. weaker intermolecular interactions occur in the liquid state and the weakest intermolecular interaction occurs in the gaseous state.
Since ammonia is a gas at room temperature, it has weaker intermolecular interaction between its molecules compared to molecules of water at room temperature:
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A chemistry student needs of isopropenylbenzene for an experiment. He has available of a w/w solution of isopropenylbenzene in acetone. Calculate the mass of solution the student should use. If there's not enough solution, press the "No solution" button.
Question:
A chemistry student needs of 10 g isopropenylbenzene for an experiment. He has available 120 g of a 42.7% w/w solution of isopropenylbenzene in acetone. Calculate the mass of solution the student should use. If there's not enough solution, press the "No solution" button.
Answer:
The answer to the question is as follows
The mass of solution the student should use is 23.42 g.
Explanation:
To solve the question we note the following
A solution containing 42.7 % w/w of isopropenylbenzene in acetone has 42.7 g of isopropenylbenzene in 100 grams of the solution
Therefore we have 10 g of isopropenylbenzene contained in
100 g * 10 g/ 42.7 g = 23.42 g of solution
Available solution = 120 g
Therefore the quantity to used from the available solution = 23.42 g of the isopropenylbenzene in acetone solution.
Two examples of energy transformations are shown. The energy transformations are similar because they both involve transformations that begin with chemical energy. Begin with electrical energy. Result in radiant energy. Result in mechanical energy.
Answer:
The answers I think you are looking for is Gasoline or Fuel (chemical energy)
Explanation:
Energy transformation involves change or conversion of energy from one form to another. Having two examples of the same form of chemical energy, convert into two or more types of energy, the best example would be gasoline.
GASOLINE/FUEL → CAR BATTERY + LIGHT BULBS (TRAFFICATOR LIGHT)
(chemical) (electrical) (radiant)
GASOLINE/FUEL → INTERNAL COMBUSTION ENGINE
(chemical) (mechanical)
Answer:
C - result in radiant energy
Explanation:
How much electrical charge does an atom with 6 protons, 6 neutrons, and 5 electrons have? How much electrical charge does an atom with 6 protons, 6 neutrons, and 5 electrons have? a total charge of +17 a negative charge of -5 a positive charge of +7 a positive charge of +1 none of the above
Answer:
a positive charge of +1
Explanation:
The charge carried by atom depends on the number of protons and electrons present. The neutrons are not charged hence they do not contribute to the net charge of the specie.
The specie mentioned in the question has six protons and five electrons. Hence it has an excess of one positive charge hence a net charge of +1.