The activation energy for the reaction NO2(g)+CO(g)⟶NO(g)+CO2(g) is Ea = 75 kJ/mol and the change in enthalpy for the reaction is ΔH = -175 kJ/mol .What is the activation energy for the reverse reaction?

Explanation:

Answer:

1.17 grams of HCl can neutralize 2.7 grams sodium bicarbonate

Explanation:

Step 1: Data given

Mass of sodium bicarbonate = 2.7 grams

Step 2: The balanced equation

HCl + NaHCO3 ⇔  NaCl + H2O + CO2

Step 3: Calculate moles NaHCO3

moles NaHCO3 =2.7 g / 84 g/mol= 0.032 moles

Step 4: Calculate moles HCl

For 1 mol NaHCO3 we need 1 mol HCl

For 0.032 moles NaHCO3 = 0.032 moles HCl

Step 5: Calculate mass HCl

Mass HCl = moles HCl * molar mass HCl

mass HCl = 0.032 * 36.46 g/mol= 1.17 grams

1.17 grams of HCl can neutralize 2.7 grams sodium bicarbonate

The key process being used here is stoichiometry, which is a core aspect of chemistry that studies the quantitative relationships, or ratios, among reactants in a chemical equation. By writing and analyzing a balanced chemical equation, performing correct conversions, and understanding mole-to-mole ratios, we determine that 2.7 grams of sodium bicarbonate can neutralize approximately 1.17 grams of hydrochloric acid.

The subject of this specific problem is stoichiometry, a central concept in chemistry. The first step involves writing a balanced chemical equation between sodium bicarbonate (NaHCO₃) and hydrochloric acid (HCl). The equation will look like this: NaHCO₃ (aq) + HCl (aq) → NaCl (aq) + CO₂ (g) + H₂O (l). This reaction demonstrates that one mole of sodium bicarbonate reacts with one mole of hydrochloric acid.

Next, we'll need to calculate the number of moles of sodium bicarbonate, using the molar mass of sodium bicarbonate, which is approximately 84 g/mol. So, 2.7 g of sodium bicarbonate equals 2.7 g / 84 g/mol = 0.0321 mol.

Since the equation shows a 1:1 ratio, this means that 0.0321 mol of sodium bicarbonate will neutralize the same amount of moles of hydrochloric acid. The molar mass of HCl is about 36.5 g/mol, so multiplying this with the moles of HCl gives the mass: 0.0321 mol * 36.5 g/mol = 1.17 g.

So, 2.7 g of sodium bicarbonate can neutralize 1.17 g of hydrochloric acid.

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Answer:

The correct answer is 21.3 J

Explanation:

The heat absorbed by water can be calculated by using the following equation:

heat= m x Sh x ΔT

Where m is the mass of water (2.46 kg= 2460 g), Sh is the specific heat capacity of water (4.18 J/g.ºC) and ΔT is the difference of temperatures (final T - initial T). We introduce this values and calculate the heat:

heat=2460 g x 4.18 J/g.ºC x (27.31ºC - 25.24ºC)

heat= 21,285.39 J

As 1 KJ= 1000 J, we must divide the answer into 1000 to obtain the heat in KJ:

21,285.39 J x 1 KJ/1000 J= 21.28 KJ≅ 21.3 KJ

Final answer:

To calculate the heat absorbed by the water, first convert the mass to grams, then find the temperature change, apply the specific heat formula, and finally convert the energy to kilojoules. The water absorbed 21.27 kJ of heat.

Explanation:

The student's question revolves around calculating the amount of heat absorbed by water when its temperature is increased. To find the quantity of heat absorbed, we use the formula q = m x c x \\u0394T, where q is the heat absorbed in joules, m is the mass of water in kilograms (which needs to be converted to grams for the specific heat value given), c is the specific heat capacity (4.18 J/g\\u00b0C for water), and \\u0394T is the change in temperature in degrees Celsius.

To solve the problem:

Convert the mass of water to grams: 2.46 kg x 1000 g/kg = 2460 g

Calculate the change in temperature: 27.31 \\u00b0C - 25.24 \\u00b0C = 2.07 \\u00b0C

Apply the formula: q = 2460 g x 4.18 J/g\\u00b0C x 2.07 \\u00b0C = 21270.44 J

Convert joules to kilojoules: 21270.44 J / 1000 = 21.27 kJ

Therefore, the water absorbed 21.27 kJ of heat.

Answer:

The formula of aspirin = [tex]C_9H_8O_4[/tex]

Explanation:

Mass of water obtained = 0.400

Molar mass of water = 18 g/mol

Moles of [tex]H_2O[/tex] = 0.400 g /18 g/mol = 0.0222 moles

2 moles of hydrogen atoms are present in 1 mole of water. So,

Moles of H = 2 x 0.0222 = 0.0444 moles

Molar mass of H atom = 1.008 g/mol

Mass of H in molecule = 0.0444 x 1.008 = 0.0448 g  

Mass of carbon dioxide obtained = 2.20 g

Molar mass of carbon dioxide = 44.01 g/mol

Moles of [tex]CO_2[/tex] = 2.20 g  /44.01 g/mol = 0.05 moles

1 mole of carbon atoms are present in 1 mole of carbon dioxide. So,

Moles of C = 0.05 moles

Molar mass of C atom = 12.0107 g/mol

Mass of C in molecule = 0.05 x 12.0107 = 0.6005 g

Given that the aspirin acid only contains hydrogen, oxygen and carbon. So,

Mass of O in the sample = Total mass - Mass of C  - Mass of H

Mass of the sample = 1.00 g

Mass of O in sample = 1.00 - 0.6005 - 0.0448 = 0.3547 g  

Molar mass of O = 15.999 g/mol

Moles of O  = 0.3547  / 15.999  = 0.0222 moles

Taking the simplest ratio for H, O and C as:

0.0444 : 0.0222 : 0.05

= 8 : 4 : 9

The empirical formula is = [tex]C_9H_8O_4[/tex]

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,  

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Mass from the Empirical formula = 9×12 + 8×1 + 16×4= 180 g/mol

The molar mass of aspirin is between 170 and 190 g/mol

So,  

Molecular mass = n × Empirical mass

170 <  n × 180 < 190

⇒ n = 1

The formula of aspirin = [tex]C_9H_8O_4[/tex]

The molecular formula for aspirin can be determined through the quantities of CO2 and H2O produced by burning it. This involves calculating the quantities of each element present and obtaining an empirical formula that must be scaled to match the molar mass of aspirin. Through this process, aspirin's molecular formula is found to be C9H8O4.

The empirical formula of aspirin can be determined by understanding the quantity of each element present in the provided quantities of Carbon Dioxide (CO2) and water (H2O) produced by burning the aspirin. From the 2.20 g of CO2, the amount of carbon is calculated to be: mass CO2 x (atomic mass of C/molar mass of CO2). Similarly, from the 0.400 g of water, the quantity of hydrogen is calculated to be: mass H2O x (2 x atomic mass of H/molar mass of H2O). The balance of the original aspirin's 1.00 g mass constitutes oxygen.

Using atomic masses (C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol), you generate the empirical formula with the simplest ratio of these elements. However, this formula will not match the molecular mass of 180.15 amu for aspirin. Therefore, a multiple is required to transform the empirical formula into the molecular formula. The required multiple is calculated as (molar mass of aspirin / molar mass of empirical formula).

Applying these calculations and steps reveals that the molecular formula for aspirin is indeed C9H8O4.

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Answer:

The atomic number of an element is: the number of protons in the nucleus of one atom.

Explanation:

The atomic number is a concept related to the structure of the atoms of each element and it is the total number of protons or elementary positive charges, of the nucleus of a certain atom.

Answer:

Option 3==> the number of protons in the nucleus of one atom.

Explanation:

In an atom, atomic number is the number of proton in the nucleus. In order to determine the number of an element in the periodic table we can make use of the number of proton in the atom that is the atomic number.

If the atoms are neutral, then the number of proton is equal to the number of electron. For instance, the neutral atom of carbon, the number of proton in it is 6 and on the periodic table or chart the 6th element is the carbon.

Answer:

Kc → 41.9

Explanation:

This is the equilibrium:

2NO₂(g) ⇌ N₂O₄(g)

So the expression for Kc will be:

Kc = [N₂O₄] / [NO₂]²

We prospose the situations:

Initially we have 1.2 moles of NO₂ and N₂O₄

X amount has reacted. As stoichiometry is 2:1, we have produced x/2 of the product during the reaction

Finally In equilibrium we have, 0.38 NO₂

                2NO₂(g)     ⇌       N₂O₄(g)

Initially        1.2                        1.2

React            x                         x/2

Eq         (1.2 - x) = 0.38          1.2 + x/2

As we have [NO₂] in the equilibrium, we can determine x (the amount that has reacted) to solve and determine, the [N₂O₄] in the equilibrium

1.2-0.38 = x → 0.82

1.2 + 0.82/2 = 2.02 → [N₂O₄]

For Kc, we need Molar concentration, so we have to divide [N₂O₄] and [NO₂] by the volume

[N₂O₄] → 2.02 mol/3L = 0.673 M

[NO₂] → 0.38 mol/3L = 0.127 M

Now we can replace the Kc expression:

Kc →  [N₂O₄] / [NO₂]² → 0.673 / 0.127² = 41.9

Remember that Kc has no UNITS

Answer:

C) 9

Math

Algebra I

Chemistry

Acid-Base Equilibrium

Step 1: Define

[OH⁻] = 1 × 10⁻⁹ M

Step 2: Find pOH

Simply take negative log₁₀ of the concentration.

Answer: The symbol of diphosphate ion is [tex]P_2O_7^{4-}[/tex]

Explanation:

An ionic compound is defined as the compound which is formed when electron gets transferred from one atom to another atom.

These are usually formed when a metal reacts with a non-metal or a metal reacts with a polyatomic ion or a reaction between two polyatomic ions takes place.

Calcium diphosphate [tex](Ca_2P_2O_7)[/tex] is formed by the combination of calcium ions [tex](Ca^{2+})[/tex] and diphosphate ions [tex](P_2O_7^{4-})[/tex]

By criss-cross method, the oxidation state of the ions gets exchanged and they form the subscripts of the other ions. This results in the formation of a neutral ionic compound.

Hence, the symbol of diphosphate ion is [tex]P_2O_7^{4-}[/tex]

Final answer:

The correct symbol for the diphosphate ion in calcium diphosphate Ca₂P₂O₇ is P₂O₇₄₋ to balance the positive charge of the two calcium ions, but the response options in the question may contain a typo. D) is correct.

Explanation:

To determine the correct symbol for the diphosphate ion, we need to consider the charge balance in the compound calcium diphosphate with the formula  Ca₂P₂O₇. Calcium has a 2+ charge (Ca₂+), and since the compound must be electrically neutral, we need to balance this charge with an appropriate anion. In this case, each calcium ion has a 2+ charge, and there are two calcium ions, resulting in a total positive charge of 4+. Therefore, the diphosphate anion must have a 4- charge in total to neutralize the charges. The correct option for the diphosphate ion is  P₂O₇₄₋, so the answer is D) P₂O₇₂₋, which accounts for two negative charges per diphosphate ion (note: this seems to be a typo in the options—the correct option should be  P₂O₇₄₋, not P₂O₇₂₋).

This is an incomplete question, here is a complete question.

Consider the following reaction:

[tex]A+B+C\rightarrow D[/tex]

The rate law for this reaction is as follows:

[tex]Rate=k\times \frac{[A][C]^2}{[B]^{1/2}}[/tex]

Suppose the rate of the reaction at certain initial concentrations of A, B, and C is 1.12 × 10⁻² M/s.

What is the rate of the reaction if the concentrations of A and C are doubled and the concentration of B is tripled?

Rate 2 = ? M/s

Answer : The rate of reaction will be, [tex]5.17\times 10^{-2}M/s[/tex]

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

The given chemical reaction is,

[tex]A+B+C\rightarrow D[/tex]

The expression of rate law for this reaction will be,

[tex]\text{ Initial rate}=k\times \frac{[A][C]^2}{[B]^{1/2}}[/tex]

As the concentrations of A and C are doubled and the concentration of B is tripled then the rate of reaction will be:

[tex]Rate=k\times \frac{[2A][2C]^2}{[3B]^1/2}[/tex]

[tex]Rate=4.62k\times \frac{[A][C]^2}{[B]^{1/2}}[/tex]

[tex]Rate=4.62\times \text{ Initial rate}[/tex]

Given:

Initial rate = 1.12 × 10⁻² M/s

[tex]Rate=4.62\times 1.12\times 10^{-2}M/s[/tex]

[tex]Rate=5.17\times 10^{-2}M/s[/tex]

Thus, the rate of reaction will be, [tex]5.17\times 10^{-2}M/s[/tex]

Answer:

0.735M

Explanation:

The balanced equation of reaction is:

HCl + KOH ===> KCl + H2O

Using titration equation of formula

CAVA/CBVB = NA/NB

Where NA is the number of mole of acid = 1 (from the balanced equation of reaction)

NB is the number of mole of base = 1 (from the balanced equation of reaction)

CA is the concentration of acid = 2.5M

CB is the concentration of base = to be calculated

VA is the volume of acid = 14.7mL

VB is the volume of base = 50mL

Substituting

2.5×14.7/CB×50 = 1/1

Therefore CB =2.5×50×1/14.7×1

CB= 0.735M

Explanation:

D(aq) + E(aq) <=> F(aq)

This question is based on Le Chatelier's principle.

Le Chatelier's principle is an observation about chemical equilibria of reactions. It states that changes in the temperature, pressure, volume, or concentration of a system will result in predictable and opposing changes in the system in order to achieve a new equilibrium state.

Increase D

D is a reactant. if we add reactants to the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.

Increase E

E is a reactant. if we add reactants to the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.

Increase F

F is a product.  If we add additional product to a system, the equilibrium will shift to the left, in order to produce more reactants. The reaction would shift to the left.

Decrease D

if we remove reactants from the system, equilibrium will  be shifted to the left.

Decrease E

if we remove reactants from the system, equilibrium will  be shifted to the left.

Decrease F

if we remove products from the system, equilibrium will be shifted to the right to in order to maintain equilibrium by producing more products.

Triple D and reduce E to one third

no shift in the direction of the net reaction, Both changes cancels each other.

Triple both E and F

no shift in the direction of the net reaction, Both changes cancels each other.

Answer:

1. 276 g of NO₂

2. 34.8 moles of LiO

3. 4.23×10²⁵ molecules of SO₂

4. 540 g of H₂O

5. 224 g CO

Explanation:

Let's define the molar mass of the compound to define the moles or the grans of each.

Molar mass . moles = Mass

Mass (g) / Molar mass = Moles

1. 6 mol . 46 g / 1 mol = 276 g of NO₂

2. 800 g . 1mol / 22.94 g = 34.8 moles of LiO

3. To determine the number of molecules, we convert the mass to moles and then, we use the NA (1 mol contains 6.02×10²³ molecules)

4500 g . 1mol / 64.06 g = 70.2 moles of SO₂

70.2 mol . 6.02×10²³ molecules / 1 mol = 4.23×10²⁵ molecules of SO₂

4. 30 mol . 18g / 1 mol = 540 g of H₂O

5. 8 mol . 28g /  1mol = 224 g CO

Answer : The empirical of the compound is, [tex]C_1H_2O_3[/tex]

Solution : Given,

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of C = 19.36 g

Mass of H = 3.25 g

Mass of O = 77.39 g

Molar mass of C = 12 g/mole

Molar mass of H = 1 g/mole

Molar mass of O = 16 g/mole

Step 1 : convert given masses into moles.

Moles of C = [tex]\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{19.36g}{12g/mole}=1.613moles[/tex]

Moles of H = [tex]\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{3.25g}{1g/mole}=3.25moles[/tex]

Moles of O = [tex]\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{77.39g}{16g/mole}=4.837moles[/tex]

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = [tex]\frac{1.613}{1.613}=1[/tex]

For H = [tex]\frac{3.25}{1.613}=2.01\approx 2[/tex]

For o = [tex]\frac{4.837}{1.613}=2.99\approx 3[/tex]

The ratio of C : H : O = 1 : 2 : 3

The mole ratio of the element is represented by subscripts in empirical formula.

The Empirical formula = [tex]C_1H_2O_3[/tex]

Therefore, the empirical of the compound is, [tex]C_1H_2O_3[/tex]

The empirical formula of a compound with 3.25% H, 19.36% C, and 77.39% O by mass is CH2O3, found by converting the mass of each element to moles and then determining the simplest whole number ratio.

To determine the empirical formula of a compound composed of 3.25% hydrogen (H), 19.36% carbon (C), and 77.39% oxygen (O) by mass, we first assume a 100 g sample of the compound. This means we would have 3.25 g of H, 19.36 g of C, and 77.39 g of O.

Next, we convert the mass of each element to moles by dividing by their respective molar masses:

To find the simplest whole number ratio, we divide each mole value by the smallest number of moles calculated:

The ratios indicate the empirical formula is CH2O3.

Answer: Thermal

Explanation: All areas on the earth surface does not absorb equal amount of sunlight, as a result of this, some areas tend to heat up more quickly than the others. The air in contact with these heated areas becomes  warmer than its surroundings causing a hot bubble of air called ''thermal'' to break away from the  warm surface,rising, expanding and cooling as it ascends, as observed during cloud development.

Final answer:

A rising hot "bubble" of air that expands and cools as it ascends due to convection is known as a thermal. This results in adiabatic cooling, which can lead to condensation and cloud formation.

Explanation:

A hot "bubble" of air that breaks away from the warm surface and rises, expanding and cooling as it ascends, is known as a thermal. This is due to the process of convection where warmer air, being less dense, rises above colder air. As this air rises, it expands due to lower atmospheric pressure at higher altitudes, which in turn causes it to cool, a process known as adiabatic cooling. If the air cools to its dew point, condensation can occur, potentially leading to cloud formation.

Answer:

a) HCl

b) 22.9g

c) 18.11g

Explanation:

MMn = 54.94g/mol

MO2 = 2(16) = 32g/mol

MH = 1g/mol

MCl = 35.45g/mol

Molar Mass of MnO2:

54.94 + 2(16)= 86.94

Molar Mass of HCl:

1+35.45=36.45

Mols of MnO2:

42.7 /86.94 = 0.49

Mols of HCl:

47.1 /36.45 = 1.29

Molar Mass of Cl2:

35.45 ×2 = 70.9

Mols of Cl2

1.29/4=0.323

Mass of Cl2 (Theoretical yield)

0.323 ×70.9= 22.9

To calculate the actual yield, we multiply the theoretical yield by the final percentage:

22.9 ×0.791=18.11

Answer:

The answer to your question is empirical formula = CH

                                                    molecular formula = C₆H₆

Explanation:

Data

Carbon  92.2%

Hydrogen  7.76%

Formula mass = 78.1 g

Process

1.- Express the percents as grams

Carbon            92.2 g

Hydrogen          7.76 g

2.- Convert the grams to moles

Carbon                 12 g ---------------- 1 mol

                            92.2 g -------------  x

                            x = (92.2 x 1)/12

                            x = 7.68 moles

Hydrogen             1 g ------------------ 1 mol

                            7.76 g -------------  x

                            x = 7.76 moles

3.- Divide by the lowest number of moles

Carbon         7.68 / 7.68 = 1

Hydrogen     7.76 / 7.68 = 1.01

4.- Write the empirical formula

                                      CH

5.- Calculate the molecular weight of the empirical formula

CH = 12 + 1 = 13

6.- Divide the molecular weight by the molecular weight of the empirical formula

                78.1 / 13 = 6

7.- Write the molecular formula

               6(CH) = C₆H₆        

The empirical formula of the compound is CH. The molecular formula of the compound is [tex]\rm \bold C_6H_6[/tex]

A molecular formula has been the one that represents the exact number of atoms in a compound. The empirical formula has been able to represent the whole number ratio of atoms present in a compound.

The given compound has 92.2% Carbon and 7.76% Hydrogen. The weight will be:

Carbon = 92.2 g

Hydrogen = 7.76 g

From the weight, the moles of elements in the compound can be calculated.

Moles = [tex]\rm \dfrac{weight}{molecular\;weight}[/tex]

Moles of carbon = [tex]\rm \dfrac{92.2}{12}[/tex]

Moles of carbon = 7.76 moles

Moles of hydrogen = weight of hydrogen

Moles of hydrogen = 7.76 moles

For the empirical formula, divide the moles of each element to the nearest mole number;

Carbon = [tex]\rm \dfrac{7.76}{7.76}[/tex]

Carbon = 1

Hydrogen = [tex]\rm \dfrac{7.76}{7.76}[/tex]

Hydrogen = 1

Thus, the empirical formula of the compound will be CH.

For finding the molecular formula, the molecular weight from the empirical formula has been divided with the molecular weight of the compound to find the number of atoms.

Molecular weight of empirical formula = weight of carbon + weight of hydrogen

Molecular weight of empirical formula = 12 + 1

Molecular weight of empirical formula = 13 grams

Molecular mass of compound = 78.1 grams.

Number of atoms of each element = [tex]\rm \dfrac{78.1}{13}[/tex]

Number of atoms of each element = 6

Thus, the molecular formula of the compound is [tex]\rm C_6H_6[/tex].

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Answer:  32.9 Liters

Explanation:

To calculate the moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}[/tex]

1. moles of [tex]FeS_2=\frac{96.7g}{119.99g/mol}=0.806mol[/tex]

2. moles of [tex]O_2[/tex]

[tex]PV=nRT[/tex]

P = pressure of the gas = 1.20  atm

R = Gas constant = [tex]0.0821\text{ L atm }mol^{-1}K^{-1}[/tex]

T = temperature of the gas = [tex]398K[/tex]

[tex]1.20\times 55.0=n\times 0.0821\times 398[/tex]

[tex]n=2.02[/tex]

[tex]4FeS_2(s)+11O_2(g)\rightarrow 2Fe_2O_3(s)+8SO_2(g)[/tex]

According to stoichiometry:

11 moles of oxygen reacts with 4 moles of [tex]FeS_2[/tex]

Thus 2.02 moles of oxygen reacts with =[tex]\frac{4}{11}\times 2.02=0.73[/tex] moles of [tex]FeS_2[/tex]

Thus oxygen acts as limiting reagent and [tex]FeS_2[/tex] is excess reagent.

As 11 moles of oxygen gives = 8 moles of [tex]SO_2[/tex]

2.02 moles of oxygen gives =[tex]\frac{8}{11}\times 2.02=1.47[/tex] moles of [tex]SO_2[/tex]

[tex]PV=nRT[/tex]

P = pressure of the gas = 1  atm (at STP)

R = Gas constant = [tex]0.0821\text{ L atm }mol^{-1}K^{-1}[/tex]

T = temperature of the gas = [tex]273K[/tex]   (at STP)

[tex]1\times V=1.47\times 0.0821\times 273[/tex]

[tex]V=32.9L[/tex]

Thus volume of [tex]SO_2[/tex] (at STP) formed from the reaction is 32.9 L

The volume of SO₂ formed from the reaction at STP is 32.92 L

From the question,

We are to determine the volume of SO₂ formed from the reaction

The given balanced chemical equation for the reaction is

4FeS₂(s) + 11O₂(g) → 2Fe₂O₃(s) + 8SO₂(g)

This means,

4 moles of FeS₂ reacts with 11 moles of oxygen to produce 2 moles of Fe₂O₃ and 8 moles of SO₂

First, we will determine the number of moles of each reactant present

Mass = 96.7 g

From the formula

[tex]Number\ of\ moles =\frac{Mass}{Molar\ mass}[/tex]

Molar mass of FeS₂ = 119.99 g/mol

∴ Number of moles of FeS₂ present =[tex]\frac{96.7}{119.99}[/tex]

Number of moles of FeS₂ present = 0.8059 mole

Using the formula

PV = nRT

[tex]n =\frac{PV}{RT}[/tex]

Putting the given parameters into the formula, we get

[tex]n = \frac{1.2 \times 55.0}{0.08206 \times 398}[/tex]

[tex]n = \frac{66}{32.65988}[/tex]

n = 2.0208 moles

Since,

4 moles of FeS₂ reacts with 11 moles of oxygen to produce 8 moles of SO₂

Then,

[tex]\frac{2.0208 \times 4}{11}[/tex] moles of FeS₂ will react with 2.0208 moles of oxygen to produce [tex]\frac{2.0208 \times 4}{11} \times 2[/tex]  moles of SO₂

That is,

0.7348 moles of FeS₂ will react with 2.0208 moles of oxygen to produce 1.4697 moles of SO₂

∴ Number of moles of SO₂ formed is 1.4697 moles

Now for the volume of SO₂ formed at STP

Since

1 mole of a gas has a volume of 22.4 L at STP

Then

1.4697 moles of the SO₂ will have a volume of 1.4697 × 22.4 L

1.4697 × 22.4 L = 32.92L

Hence, the volume of SO₂ formed from the reaction at STP is 32.92 L

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Answer:

Option (E) is correct

Explanation:

Solubility equilibrium of [tex]Pb(IO_{3})_{2}[/tex] is given as follows-

                   [tex]Pb(IO_{3})_{2}\rightleftharpoons Pb^{2+}+2IO_{3}^{-}[/tex]

Hence, if solubility of [tex]Pb(IO_{3})_{2}[/tex] is S (M) then-

                             [tex][Pb^{2+}]=S(M)[/tex] and [tex][IO_{3}^{-}]=2S(M)[/tex]

Where species under third bracket represent equilibrium concentrations

So, solubility product of [tex]Pb(IO_{3})_{2}[/tex] , [tex]K_{sp}=[Pb^{2+}][IO_{3}^{-}]^{2}[/tex]

Here, [tex][Pb^{2+}]=S(M)=5.0\times 10^{-5}M[/tex]

So, [tex][IO_{3}^{-}]=2S(M)=(2\times 5.0\times 10^{-5})M=1.0\times 10^{-4}M[/tex]

So, [tex]K_{sp}=(5.0\times 10^{-5})\times (1.0\times 10^{-4})^{2}=5.0\times 10^{-13}[/tex]

Hence option (E) is correct

Answer:

E) 5 x 10-13 Molar

Explanation:

plato

Answer : The final concentration of [tex]N_2O_5[/tex] is, 2.9 M

Explanation :

Expression for rate law for first order kinetics is given by:

[tex]t=\frac{2.303}{k}\log\frac{a}{a-x}[/tex]

where,

k = rate constant  = [tex]5.89\times 10^{-3}\text{ min}^{-1}[/tex]

t = time passed by the sample  = 3.5 min

a = initial concentration of the reactant  = 3.0 M

a - x = concentration left after decay process = ?

Now put all the given values in above equation, we get

[tex]3.5=\frac{2.303}{5.89\times 10^{-3}}\log\frac{3.0}{a-x}[/tex]

[tex]a-x=2.9M[/tex]

Thus, the final concentration of [tex]N_2O_5[/tex] is, 2.9 M

To determine the final concentration of N2O5 after 3.5 minutes using the provided rate constant and first-order kinetics, the integrated rate law is used, where the time is converted to seconds and calculations are made using the initial concentration, resulting in a final concentration of 0.17 M.

The student is asking about the final concentration of N2O5 after a first-order decomposition reaction where the initial concentration and rate constant are provided. To find the final concentration of N2O5 after a period of 3.5 minutes, we use the first-order integrated rate law:

ln[A] = -k * t + ln[A0]

Where:

Since the time given is in minutes, we first convert it to seconds: t = 3.5 min × 60 s/min = 210 s. Now we can use the integrated rate law to find the final concentration:

ln[3.0] = -5.89 × 10⁻³ × 210 + ln[3.0]

Solving for [A], we find that the final concentration of N2O5 is 0.17 M (using appropriate exponential and logarithmic operations).

Answer:

The molal boiling point elevation constant (Kb) is calculated by dividing the change in boiling point (∆Tb) by the molality of the solution (m)

Explanation:

Kb = ∆Tb/m

Kb is the molal boiling point elevation constant of the liquid

∆Tb is the change in boiling point. It is calculated by subtracting the initial boiling point of the liquid from the final boiling point of the solution.

m is the molality of the solution. It is calculated by dividing the number of moles of urea (number of moles of urea is calculated by dividing the mass in grams of urea by its molecular weight) by the mass of the liquid in kilograms.

Explanation:

It is known that specific heat of water is 4.184 [tex]J/g^{o}C[/tex] and atomic mass of tin is 118.7 g/mol. For the given situation,

                 [tex]Q_{lost} = Q_{gained}[/tex]

Let us assume that,

               [tex]m_{1}[/tex] = mass of Sn

               [tex]m_{2}[/tex] = mass of [tex]H_{2}O[/tex]  

Therefore, heat energy expression for heat lost and gained is as follows.

           [tex]Q_{lost} = Q_{gained}[/tex]

      [tex]m_{1}C_{1}(T_{2} - T_{1}) = m_{2}C_{2}(T_{1} - T_{2})[/tex]

   [tex]100 g \times C_{1} \times (100^{o}C - 27.4^{o}C) = 150 g \times 4.184 /g^{o}C \times (27.4^{o}C - 25^{o}C)[/tex]

           [tex]7260C_{1} = 150 \times 4.184 \times 2.4[/tex]

                 [tex]C_{1} = \frac{1506.24}{7260}[/tex]

                              = 0.207 [tex]J/g^{o}C[/tex]

For, 118.7 g the specific heat of tin will be calculated as follows.

               [tex]C_{1} = 0.207 J/g^{o}C \times 118.7 g[/tex]

                          = 24.5 [tex]J/mol^{o}C[/tex]

Thus, we can conclude that specific heat of tin is 24.5 [tex]J/mol^{o}C[/tex].

To calculate the specific heat capacity of the metal, we can use the equation q = m * c * ΔT, where q is the heat transferred, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. By using the known temperatures and masses of the metal and water, we can solve for the specific heat capacity of the metal.

To calculate the specific heat capacity of the metal, we can use the equation q = m * c * ΔT, where q is the heat transferred, m is the mass, c is the specific heat capacity, and ΔT is the change in temperature. In this case, we know the initial and final temperatures of the metal and water, as well as the masses of the metal and water. We can rearrange the equation to solve for the specific heat capacity of the metal, c.

We can start by calculating the heat transferred from the metal to the water. The heat transferred to the water can be calculated using the equation q_water = m_water * c_water * ΔT_water, where m_water is the mass of the water, c_water is the specific heat capacity of water, and ΔT_water is the change in temperature of the water.

Next, we can calculate the heat transferred from the metal to the water using the equation q_metal = m_metal * c_metal * ΔT_metal, where m_metal is the mass of the metal, c_metal is the specific heat capacity of the metal, and ΔT_metal is the change in temperature of the metal.

Since the metal and water reach the same final temperature, we can set q_water equal to q_metal and solve for the specific heat capacity of the metal, c_metal.

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Answer:

Catalysis

Explanation:

Pepsin is able to break peptide bonds, turning large protein molecules into small peptide chains.

When pepsin acts to break down pepsinogen (inactive form of pepsin), it is accelerating pepsinogen → pepsin reactions, acting as a catalyst, reducing activation energy and favoring proteolytic reactions at a higher rate.

This process of accelerating reactions is characteristic of enzymes and is known as catalysis.

Answer:

A

Explanation:

During a chemical reaction two or more chemical substances interact with one another, causing the atoms to move around and rearrange their arraignment and bond together in a different way to make a new product or products.

Answer:

A

Explanation:

One of the principal laws guiding chemical reactions is the law of conservation of mass. It states that matter can not be created nor destroyed but can be converted from one form to another. Although this has been shown to be wrong to an extent, it is still the basic law guiding the way in which chemical reactions operate.

Now, to form new substances, we have some old substances coming together. These old substances are the ones that come together to form the new ones. Surely, these old substances have their own atoms too. Since they are not destroyed in the process of forming new substances, what will happen is that they are rearranged or converted from their original form to another new form to make way for the emergence of new substance type.

Answer:

B. It is important that people are not harmed for the sake of science.

Explanation:

Ethical principles stress the need to do good and cause no harm.A researcher is therefore required to;

Answer:

It is important that people are not harmed for the sake of science.

Explanation:

Answer:

                                   Δ            

            CaCO3(s)     →  →      CaO (s)   +  CO2 (g)

Explanation: Calcium Carbonate also known as Limestone will undergo decomposition reaction in the presence of heat to produce Quick-lime and Carbon dioxide.

Answer:

The balanced chemical equation is:

[tex]CaCO_{3}[/tex]  →  [tex]CaO + CO_{3}[/tex]

Explanation:

The problem said:

Solid calcium carbonate decomposes into solid calcium oxide and carbon dioxide gas.

Corresponde to chemicale equation:

                                               [tex]CaCO_{3}[/tex]   →  [tex]CaO + CO_{3}[/tex]

A chemical reaction must be based on the law of the conservation of matter, which implies that matter is not created or destroyed but transformed. Therefore, the same amount of each atom must be involved in the reagents and products.

this reaction have:

Reagents.

Products.

∴ This equation is balanced.

Answer:

The answer to your question is  T = 204.9°K

Explanation:

Data

Temperature = T = ?

number of moles = n = 4

Volume = V = 12 L

Pressure = P = 5.60 atm

constant of gases = 0.082 atm L /mol °K

Process

To solve this problem, use the Ideal Gas Law and solve it for T

Formula

            PV = nRT

            T = PV / nR

-Substitution

             T = (5.60)(12)/(4)((0.082)

-Simplification

              T = 67.2 / 0.328

-Result

               T = 204.9°K

Considering the ideal gas law, at 204.878 K will 4.00 moles of gas occupy a volume of 12.0 L at a pressure of 5.60 atm.

An ideal gas is a theoretical gas that is considered to be composed of randomly moving point particles that do not interact with each other. Gases in general are ideal when they are at high temperatures and low pressures.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:  

P×V = n×R×T

where P is the gas pressure, V is the volume that occupies, T is its temperature, R is the ideal gas constant, and n is the number of moles of the gas. The universal constant of ideal gases R has the same value for all gaseous substances. The numerical value of R will depend on the units in which the other properties are worked.

In this case, you know:

Replacing in the ideal gas law:

5.60 atm×12  L = 4 moles×0.082[tex]\frac{atmL}{molK}[/tex]×T

Solving:

[tex]T=\frac{5.60 atmx12 L}{4 moles x 0.082 \frac{atmL}{molK}}[/tex]

T=204.878 K

Finally, at 204.878 K will 4.00 moles of gas occupy a volume of 12.0 L at a pressure of 5.60 atm.

Learn more about the ideal gas law:

Answer:

in nuclear fusion deep in the interiors of stars

Explanation:

Nuclear fusion -

It is the type of reaction , where two or more atomic nuclei of the atom merges together to release two or more different nuclei along with some subatomic particles , is referred to as a nuclear fusion reaction .

The reaction can very well be done on stars , because of very high energy .

Hence , a nuclear fusion occurs deep inside the stars .

Answer:

5 g/dm³ is the correct answer

Explanation:

Concentration in units of g/dm³ means the grams of solute, in 1 dm³ of solution.

We can make a rule of three:

In 2 dm³ of solution we have 10 g of NaCl

Therefore, 1 dm³ of solution we would have (1dm³ . 10g) / 2dm³ = 5g

If we were asked for concentration of g/dm³ we can also make this division:

10 g / 2dm³ = 5g/dm³

The 10.0 g of NaCl in 2.00 dm³ of water results in a concentration of 5.0 g/dm³.

To find the concentration of the solution in units of g/dm³, use the formula:

Given:

Now, plug in the values:

Therefore, the concentration of the sodium chloride solution is 5.0 g/dm³.

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Answer:

decreases going down within a group

Explanation:

Ionization energy of an atom is defined as the energy required to remove electron from the gaseous form the atom. The energy required to remove the highest placed electron in the gaseous form of an atom is referred to as the first ionization energy.

In the periodic table, the first ionization energy decreases down the group because as the principal quantum number increases, the size of the orbital increases and the electron is easier to remove.

In addition, the first ionization energy increases across the period because electrons in the same principal quantum shell do not completely shield the increasing nuclear charge of the protons.

The ionization energy of atoms decreases going down a group on the periodic table and increases going across a period. This is because the atomic radius and the attraction between the nucleus and the outer electrons change.

The ionization energy of atoms is the energy required to remove an electron from an atom or ion. As you move down a group on the periodic table, the ionization energy generally decreases. This is because as you go down a group, the atomic radius increases and the outer electrons are further away from the nucleus, making them easier to remove.

On the other hand, as you go across a period from left to right, the ionization energy generally increases. The electrons are closer to the nucleus and thus more strongly attracted to the center, making them more difficult to remove. So, the correct choices would be 'decreases going down within a group' and 'increases going across a period'.

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Answer: The total pressure inside the container is 77.9 kPa

Explanation:

Dalton's law of partial pressure states that the total pressure of the system is equal to the sum of partial pressure of each component present in it.

To calculate the total pressure inside the container, we use the law given by Dalton, which is:

[tex]P_T=p_{N_2}+p_{O_2}+p_{Ar}[/tex]

We are given:

Vapor pressure of oxygen gas, [tex]p_{O_2}[/tex] = 40.9 kPa

Vapor pressure of nitrogen gas, [tex]p_{N_2}[/tex] = 23.3 kPa

Vapor pressure of argon, [tex]p_{Ar}[/tex] = 13.7 kPa

Putting values in above equation, we get:

[tex]p_T=23.3+40.9+13.7\\\\p_{T}=77.9kPa[/tex]

Hence, the total pressure inside the container is 77.9 kPa