Consider the steps in coal gasification: C(coal) + H2O(g) → CO(g) + H2(g) ΔH°rxn = 129.7 kJ CO(g) + H2O(g) → CO2(g) + H2(g) ΔH°rxn = -41 kJ CO(g) + 3H2(g) → CH4(g) + H2O(g) ΔH°rxn = -206 kJ Calculate the heat of reaction, ΔH°rxn, for overall reaction for the production of methane, CH4.

Answer:

a. 100:11

Explanation:

M+1 peak is observed due to the presence of an isotope of an atom in a molecule. Decane has the molecular formula C₁₀H₂₂, so the probability of having 13C atom in this molecule increases ten times. This gives the ratio between M+ and M+1 peak 100:11.

It should be noted that the decane molecule also contains hydrogen atoms whose isotope deuterium (2H) can also be present in the molecule and give M+1 peak. But its relative abundance to protium (1H) is low i.e., 0.015, so its effect can be neglected.

A simple formula for the estimation of the relative peak height of M+1 in a molecule that contains C, H, N, O, F, Si, P, and S is:

[tex][M+1] = (number of C X 1.1) + (number of H X 0.015) + (number of N X 0.37) + (number of O X 0.04) + (number of S X 0.8) + (number of Si X 5.1)[/tex]

PS: remove the element from the formula which is not present in the molecule

Answer:

the final temperature T final = 83.863 °C

Explanation:

Assuming that no heat is absorbed from the container , then all the heat absorbed by the water Q water comes from the heat released by the quartz (-Q quatz), since

Q water + Q quatz = Q surroundings =0

denoting w as water and q as quartz then

Q water = mw * cpw * (Tfinal - T initial w)

Q quartz = mq * cpq * (Tfinal - T initial q)

where

m= mass

cp= specific heat capacity at constant pressure

T final = final temperature

T initial w and T initial q = initial temperature of water and quartz respectively

then

mw * cpw * (Tfinal - T initial w) + mq * cpq * (Tfinal - T initial q) = 0

mw * cpw * Tfinal + mq * cpq * Tfinal = mw * cpw *T initial w + mq * cpq * T initial q

Tfinal = (mw * cpw *T initial w+ mq * cpq * T initial q)/(mw * cpw +mq * cpq)

replacing values and assuming cpw= 1 cal/gr°C = 4.186 J/g°C

Tfinal = (200 g * 4.186 J/g°C * 85 °C + 17g * 0.730 J/g°C * 7.2 °C)/(200 g * 4.186 J/g°C + 17g * 0.730 J/g°C) = 83.863 °C

Tfinal = 83.863 °C

Answer:

The mass of xenon in the compound is 2.950 grams

Explanation:

Step 1: Data given

Mass of XeF4 = 4.658 grams

Molar mass of XeF4 = 207.28 g/mol

Step 2: Calculate moles of XeF4

Moles XeF4 = mass XeF4 / molar mass XeF4

Moles XeF4 = 4.658 grams / 207.28 g/mol

Moles XeF4 = 0.02247 moles

Step 3: Calculate moles of xenon

XeF4 → Xe + 4F-

For 1 mol xenon tetrafluoride, we have 1 mol of xenon

For 0.02247 moles XeF4 we have 0.02247 moles Xe

Step 4: Calculate mass of xenon

Mass xenon = moles xenon * molar mass xenon

Mass xenon = 0.02247 moles * 131.29 g/mol

Mass xenon = 2.950 grams

The mass of xenon in the compound is 2.950 grams

To calculate the number of grams of xenon in 4.658 g of xenon tetrafluoride, we need to determine the molar mass of XeF4 and convert grams to moles. The molar mass of XeF4 is 207.282 g/mol. Using this molar mass, we find that there are 0.0225 moles of XeF4, which corresponds to 2.968 grams of xenon.

To calculate the number of grams of xenon in 4.658 g of xenon tetrafluoride, we need to first determine the molar mass of xenon tetrafluoride (XeF4) and then use it to convert grams to moles. The molar mass of XeF4 is calculated as follows:

Molar mass of Xe = 131.293 g/mol

Molar mass of F = 18.998 g/mol

Molar mass of XeF4 = (131.293 g/mol) + 4 * (18.998 g/mol) = 207.282 g/mol

Now, we can use the molar mass to convert grams to moles:

Moles of XeF4 = (4.658 g) / (207.282 g/mol) = 0.0225 mol

Finally, we can convert moles of XeF4 to grams of xenon:

Grams of xenon = (0.0225 mol) * (131.293 g/mol) = 2.968 g

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The question is incomplete, here is the complete question:

In the Minnesota Department of Health set a health risk limit for methanol in groundwater of 4.00 μg/L. Suppose an analytical chemist receives a sample of groundwater with a measured volume of 76.0 mL.

Calculate the maximum mass in milligrams of methanol which the chemist could measure in this sample and still certify that the groundwater from which it came met Minnesota Department of Health standards. Be sure your answer has the correct number of significant digits.

Answer: The risk limit of methanol in the given amount of methanol is [tex]3.04\times 10^{-4}mg[/tex]

Explanation:

We are given:

Risk limit for methanol in groundwater = 4.00 μg/L = 0.004 mg/L    (Conversion factor:  [tex]1mg=1000\mu g[/tex] )

Volume of groundwater that is to be measured = 76.0 mL

We know that:

1 L = 1000 mL

Applying unitary method:

In 1000 mL of groundwater, the risk limit of methanol is 0.004 mg

So, in 76.0 mL of groundwater, the risk limit of methanol will be = [tex]\frac{0.004}{1000}\times 76.0=3.04\times 10^{-4}mg[/tex]

Hence, the risk limit of methanol in the given amount of methanol is [tex]3.04\times 10^{-4}mg[/tex]

Answer:

Answers explained below

Explanation:

(a)Given,

Molecular formula of the complex = [Ni(NH3)x(H2O)y]Clz

(i) Ni is in +2 oxidation state in the complex.

(ii) NH3 and H2O are the neutral ligands but Cl  is the negatively charged ligand.

(iii) complex is neutral

So, to make the nickel complex in +2 oxidation with neutral charge, we requires 2 Cl-.

Hence, form the above statements, we can say that here in the complex

z=2

(b) Molarity of HCl = 0.2005M

Volume of HCl used = 20.02mL = 20.02*10-3 L

Weight of the nickel(II) ammonia complex = 0.1550g

Reaction of HCl with Ammonia,

HCl (aq) + NH3 (aq) -> NH4Cl (aq)

HCl reacts with ammonia in 1:1 ratio to form ammonium salt (NH4Cl). That means 1 mol of HCl reacts with 1 mol of NH3.

So, we have to find number of moles of HCl used.

No. of moles of HCl used = Molarity of HCl * Volume of HCl used (L)

= 0.2005M * 20.02*10-3 L = 4.014*10-3 moles

Hence no. of moles of ammonia in the complex = No. of moles of HCl used = 4.014*10-3 mol

So, Experimental Equivalent Weight = Weight of the nickel(II) ammonia complex/ No. of moles of NH3

= 0.1550g / 4.014*10-3 mol

= 38.615 g/mol

Hence, Experimental Equivalent Weight = 38.615 g/mol

(c) Given,

x+y=< 6

Molar mass of [Ni(NH3)x(H2O)y]Clz = 58.69 + x(14.00+3*1) + y(16+2*1)+z(35.45)

= (58.69 + 17x + 18y + 35.45z) g/mol

Case1 x=6, y=0 and z=2

Molar mass of [Ni(NH3)6(H2O)0]Cl2   = (58.69 + 17*6 + 18*0 + 35.45*2) g/mol

= 58.69+102+70.90 = 231.59 g/mol

Experimental Equivalent Weight = 233.59/6 = 38.598 g/mol

So, This experimental equivalent weight is equal to the calculated experimental equivalent weight.

Hence the molecular formula of the complex is [Ni(NH3)6]Cl2 where x=6, y=0 and z=2.

Note: You can try other combination but in every case you will find lower or higher calculated experimental equivalent weight.

Answer: The formula of the compound formed between rubidium and fluorine is RbF

Explanation:

Ionic bond is defined as the bond which is formed by complete transfer of electrons from one atom to another atom.

The atom which looses the electron is known as electropositive atom and the atom which gains the electron is known as electronegative atom. This bond is usually formed between a metal and a non-metal.

Rubidium is the 37th element of the periodic table having electronic configuration of [tex]1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^1[/tex]

This will loose 1 electron to form [tex]Rb^+[/tex] ion

Fluoride is the 9th element of the periodic table having electronic configuration of [tex]1s^22s^22p^5[/tex]

This will gain 1 electron to form [tex]F^-[/tex] ion

To form [tex]RbF[/tex] compound, 1 rubidium ion is needed to neutralize the charge on fluoride ion

The formation of the given compounds is shown in the image below.

Explanation:

Relation between [tex]k_{f}[/tex], molality and temperature is as follows.

                 T = [tex]K_{f} \times m \times i[/tex]

It is also known as depression between freezing point where, i is the Van't Hoff factor.

Let us assume that there is 100% dissociation. Hence, the value of i for these given species will be as follows.

          i for [tex]CaCl_{2}[/tex] = 3

           i for glucose = 1

           i for NaCl = 2

Depression in freezing point will have a negative sign. Therefore, d

depression in freezing point for the given species is as follows.

        [tex]T_{CaCl_{2}} = -1.86 \times 0.45 \times 3[/tex]

                  = [tex]-2.511^{o}C[/tex]

        [tex]T_{glucose} = 1.86 \times 0.45 \times 1[/tex]

                   = [tex]-0.837^{o}C[/tex]

       [tex]T_{NaCl} = -1.86 \times 0.45 \times 2[/tex]

                    = [tex]-1.674^{o}C[/tex]

Therefore, we can conclude that given species are arranged according to their freezing point depression with the least depression first as follows.

                     Glucose < NaCl < [tex]CaCl_{2}[/tex]

Answer:

0.102 cal/g.°C

Explanation:

According to the law of conservation of energy, the sum of the heat released by the electric burner (Qb) and the heat absorbed by the water (Qw) is zero.

Qb + Qw = 0

Qb = -Qw

Both heats can be calculated using the following expression.

Q = c × m × ΔT

where,

c: specific heat

m: mass

ΔT: change in the temperature

Then,

Qb = -Qw

cb × mb × ΔTb = - cw × mw × ΔTw

cb = - cw × mw × ΔTw / mb × ΔTb

cb = - (1 cal/g.°C) × 552.0 g × (80.3°C - 23.2°C) / 683.0 g × (23.2°C - 477.6°C)

cb = 0.102 cal/g.°C

Answer: e) all of these

Explanation:

Element is a pure substance which is composed of atoms of similar elements.It can not be decomposed into simpler constituents using chemical reactions.Example: Copper

Compound is a pure substance which is made from atoms of different elements combined together in a fixed ratio by mass.It can be decomposed into simpler constituents using chemical reactions. Example: water  [tex](H_2O)[/tex], carbon dioxide [tex](CO_2)[/tex]

Mixtures are not pure substances as they consist of elements and compounds combined physically and not in any fixed ratio. Example: Air

Thus all given substances are pure substances.

Final answer:

The correct answer to the example of a pure substance is e) all of these, which includes elements, compounds, water (H₂O), and carbon dioxide (CO₂).

Explanation:

An example of a pure substance can be any of the following: a) an element, b) a compound, c) H₂O (which is water, a compound), and d) carbon dioxide (also a compound). Therefore, the correct answer to the question is e) all of these.

A pure substance has a constant composition and characteristic properties. Each element is made up of one type of atom, and cannot be broken down further by chemical means. Examples include carbon and oxygen. On the other hand, a compound is constituted by two or more elements chemically bonded in a fixed ratio, such as water (H₂O) and carbon dioxide (CO₂).

Answer:

a) 0.046 mol/L

b) 0.016 mol

c) 271.58 g/mol

Explanation:

A nonelectrolyte solute is a solute that, when dissolved in a solvent, will not make the solution a conductor, and so the electricity will not pass through it. The osmotic pressure is a colligative property, and it's the pressure difference needed to stop the flow of a solution across a semipermeable membrane. It can be calculated by:

π = MRT

Where π is the osmotic pressure, M is the molarity of the solute (mol/L), R is the ideal gas constant, and T is the temperature (in K). For a pressure in torr, R = 62.3637 torr.L/(mol.K).

a) π = MRT , T = 25°C = 298 K

851 = M*62.3637*298

18584.3826M = 851

M = 0.046 mol/L

b) The number of moles of the solute (n) is the molar concentration (molarity) multiplied by the volume. So, for a solution of 345 mL = 0.345 L,

n = 0.046 * 0.345

n = 0.016 mol

c) The molar mass (MM) is the mass divided by the number of moles:

MM = 4.31/0.016

MM = 271.58 g/mol

The temperature at which zirconium becomes superconducting in degrees Celsius is approximately 272.85°C.

To convert the temperature from millikelvin (mk) to degrees Celsius (°C), we need to use the formula:

T(°C) = T(mk) - 273.15

Applying this formula to the given temperature of 546 mk:

T(°C) = 546 - 273.15 = 272.85°C

Therefore, the temperature at which zirconium becomes superconducting in degrees Celsius is approximately 272.85°C.

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Answer:

B

Explanation:

Carbon is an element with an atomic number 6, the electron configuration is 2,4. This means it has four electrons in its outer-most shell or valence shell. The valence shell needs 8 electrons to be filled. Thus the outer electron shell of carbon is unfilled.

It reacts with other elements covalently and forms organic and in-organic compounds.

The 4 electrons in the valance shell of carbon makes it a metalliod, but commonly its considered as a non-metal.

However carbon can form single and double covalent bonds. It forms single covalent bond when it combines with 4 atoms of Hydrogen in the methane molecule

Carbon's possession of four valence electrons allows it to form up to four single covalent bonds with other atoms, making it highly versatile and reactive in the formation of various compounds. It does not have a filled outer electron shell, and it is not positively charged.

The correct answer is option B.

Carbon has four electrons in its outer electron shell, which is also known as the valence shell. This electron configuration plays a crucial role in carbon's chemical behavior and its ability to form a wide variety of compounds. Let's examine the given options:

a. it has a filled outer electron shell: This statement is incorrect. A filled outer electron shell for carbon would require eight electrons in its valence shell, following the octet rule. Carbon only has four valence electrons, so its outer shell is not filled.

b. it can form four single covalent bonds: This statement is correct. Carbon has four valence electrons, which allows it to form up to four single covalent bonds with other atoms. This ability to form multiple bonds is a fundamental characteristic of carbon and is the basis for the vast diversity of organic compounds found in nature.

c. it does not react with any other atoms: This statement is incorrect. Carbon is highly reactive and readily forms compounds through covalent bonding with other elements, especially hydrogen, oxygen, nitrogen, and other carbon atoms. Its reactivity is a key feature that makes carbon the foundation of organic chemistry.

d. it has a positive charge: This statement is incorrect. Carbon, like all neutral atoms, has a balanced number of protons and electrons, resulting in no net electrical charge. It is neither positively charged (cation) nor negatively charged (anion).

Therefore, from the given options the correct one is B.

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B. The salt bridge will become weaker.

Therefore, the salt bridge will become weaker, so option B is correct.

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The salt bridge between glutamic acid and histidine will be unaffected as the pH increases from pH 6.9 to pH 7.5.

The salt bridge between glutamic acid and histidine will be unaffected as the pH increases from pH 6.9 to pH 7.5.

Glutamic acid has a pKa of 4.2, meaning that at pH 6.9, the glutamic acid side chain will be in its deprotonated form, which is negatively charged. Histidine has a pKa of 6.5, so at pH 6.9, the histidine side chain will be in its protonated form, which is positively charged.

As the pH increases to 7.5, both glutamic acid and histidine will become less charged, but the relative charges of the two side chains will remain the same, thus the salt bridge between them will be unaffected.

Answer:

B:COTYLEDONS

Explanation:

Cotyledon is defined as;it is the part of embryo present whithin the seed of a plant and is often referred as "seed leaf"

The number of cotyledons is a defining characteristic of angiosperms.Cotyledons are present in the embryo of the angiosperms.On the basis of the number of cotyledons ;angiosperms are divided or distinguished into two classes which are termed as;Monocotyledonae (Monocots) and Dicotyledonae (Dicots).

MONOCOTS

The species which have one cotyledon in their seeds are monocots.corn,wheat,barley,rice.

DICOTS

The species having two cotyledons are called dicots.peas,beans,peanuts.

Yup. It's B, Cotyledons. I got it right on edge 2020

Answer:

Explanation: The lowest pressure in a laboratory is 4.0×10^-11Pa

Using Ideal gas equation

PV = nRT

P= 4.0×10^-11Pa

V= 0.020m^3

T= 20+273= 293k

n=number of moles = m/A

Where m is the number of molecules and A is the Avogradro's number=6.02×10²³/mol

R=8.314J/(mol × K)

PV= m/A(RT)

4.0×10^-11 ×0.020 = m/6.02×10²³(8.314×293)

m = 4.0×10^-11×0.020×6.02×10^23 / (8.314×293)

m = 1.98×10^8 molecules

Therefore,the number of molecules is 1.98×10^8

Answer:

The student should use 156.7 g of solution

Explanation:

31.9 %w solution of acetic acid in ethanol means 100 g of solution contains 31.9 g of acetic acid.

So, 450. g of solution contains [tex](\frac{31.9\times 450.}{100})g[/tex] of acetic acid or 143.55 g of acetic acid

Alternatively, 143.55 g of acetic acid is present in 450. g of solution

So, 50.00 g of acetic acid is present in [tex](\frac{450.\times 50.00}{143.55})g[/tex] solution or 156.7 g of solution

Hence the student should use 156.7 g of solution

Answer:

Density of CO₂ at STP = 1.96 g/L

Explanation:

1 mol of any gas at STP occupies 22.4L of volume.

The rule for the Ideal gases.

Assume 1 mol of CO₂, we know that has 44 grams of mass.

Density = mass / volume

44 g/ 22.4L = 1.96 g/L

Answer: 1.96g/L

Explanation:

1mole of CO2 contains 22.4L at stp.

1mole of CO2 = 12 + ( 2x16) = 12 + 32 = 44g

Density = Mass /volume

Density = 44g /22.4L

Density = 1.96g/L

Answer:

Mass of heptane = 102g

Vapor pressure of heptane = 454mmHg

Molar mass of heptane = 100.21

No of mole of heptane = mass/molar mass = 102/100.21

No of mole of heptane = 1.0179

Therefore the partial pressure of heptane = no of mole heptane *Vapor pressure of heptane

Partial pressure of heptane = 1.0179*454mmHg

Partial pressure of heptane = 462.1096 = 462mmHg

the partial pressure of heptane vapor above this solution = 462mmHg

The partial pressure of the heptane vapor above the solution is calculated using Raoult's law as 214.5 mmHg.

In order to calculate the partial pressure, we will use Raoult's law, which states that the partial pressure of a component in a mixture is equal to the vapor pressure of the pure component multiplied by its mole fraction in the mixture. First, we need to calculate the mole fraction, which is calculated as:

moles of component/total moles in the mixture.

We first need to determine the number of moles of heptane and chloroform, using their respective molecular weights (C₇H₁₆ is approximately 100.21 g/mol, CHCl₃ is about 119.38 g/mol).

Moles of C₇H₁₆ = 102 g / 100.21 g/mol = 1.018 mol

Moles of CHCl₃= 135 g / 119.38 g/mol = 1.131 mol

To determine the mole fraction of the heptane, we take the moles of heptane and divide by the total moles.

X_C₇H₁₆ = 1.018 mol / (1.018 mol + 1.131 mol) = 0.473

Applying Raoult's law, the partial pressure of heptane P_C₇H₁₆ = X_C₇H₁₆ ₓ P(C₇H₁₆, pure) = 0.473 ₓ 454 mmHg = 214.5 mmHg.

So, the partial pressure of heptane vapor above the solution is 214.5 mmHg.

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To classify molecules as polar or nonpolar, we need to consider molecular geometry and polarity of bonds.

In order to determine if a molecule is polar or nonpolar, we need to look at the molecular geometry and the polarity of the individual bonds within the molecule. If the molecule has polar bonds and is asymmetrical in shape, it will be polar. If the molecule has either nonpolar bonds or is symmetrical in shape, it will be nonpolar.

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Answer:

The empirical formula is = [tex]CCl_3[/tex]

The molecular formula = [tex]C_2Cl_6[/tex]

Explanation:

[tex]Moles =\frac {Given\ mass}{Molar\ mass}[/tex]

% of C = 10.13

Molar mass of C = 12.0107 g/mol

% moles of C = 10.13 / 12.0107 = 0.8434

% of Cl = 89.87

Molar mass of Cl = 35.453 g/mol

% moles of Cl = 89.87 / 35.453 = 2.5349

Taking the simplest ratio for C and Cl as:

0.8434 : 2.5349

= 1 : 3

The empirical formula is = [tex]CCl_3[/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 = 12*1 + 3*35.5 = 118.5 g/mol

Molar mass = 237 g/mol

So,  

Molecular mass = n × Empirical mass

237 = n × 118.5

⇒ n ≅ 2

The molecular formula = [tex]C_2Cl_6[/tex]

1. The empirical formula of the compound containing 10.13% C and 89.87% Cl is CCl₃

2. The molecular formula of the compound is C₂Cl₆

Divide by their molar mass

C = 10.13 / 12 = 0.844

Cl = 89.87 / 35.5 = 2.532

Divide by the smallest

C = 0.844 / 0.844 = 1

Cl = 2.532 / 0.844 = 3

Thus, the empirical formula of the compound is CCl₃

Molecular formula = n × empirical = molar mass

[CCl₃]n = 237

[12 + (3×35.5)]n = 237

118.5n = 237

Divide both side by 118.5

n = 237 / 118.5

n = 2

Molecular formula = [CCl₃]n

Molecular formula = [CCl₃]₂

Molecular formula = C₂Cl₆

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The question is incomplete, here is the complete question:

A chemist measures the amount of bromine liquid produced during an experiment. She finds that 766.g of bromine liquid is produced. Calculate the number of moles of bromine liquid produced. Round your answer to 3 significant digits.

Answer: The amount of liquid bromine produced is 4.79 moles.

Explanation:

To calculate the number of moles, we use the equation:

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

We are given:

Given mass of liquid bromine = 766. g

Molar mass of liquid bromine, [tex](Br_2)[/tex] = 159.8 g/mol

Putting values in above equation, we get:

[tex]\text{Moles of liquid bromine}=\frac{766.g}{159.8g/mol}=4.79mol[/tex]

Hence, the amount of liquid bromine produced is 4.79 moles.

Answer: helps them survive

Explanation: because they want to and need to

Answer:

H+  ----- Br-

H+  ----- Cl-

O₋₋ -----2H++

CH3 ----- O-   ------ H+

Explanation:

Dipole moment occurs when there is bonding between a very strong electronegative element and hydrogen atom.

Electronegative elements are the element which attract electrons towards themselves, (that is they have strong affinity for electrons).

Generally, group 7 elements (Fluorine, Chlorine, Bromine, Iodine) of the periodic table are highly electronegative

In HBr, HCI, and H2O, there are polar covalent bonds resulting in dipole moments

(a) HBr: H-Br bond is polar covalent. The dipole moment points from Br (delta negative) to H (delta positive).

(b) HCI: H-Cl bond is polar covalent. The dipole moment points from Cl (delta negative) to H (delta positive).

(c) H2O: O-H bonds are polar covalent. The dipole moments point from O (delta negative) to H (delta positive).

(d) CH40: No polar covalent bonds. The dipole moments cancel each other out due to the symmetrical arrangement of the atoms.

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Answer:

4-chloro-4-methyl-cyclohexene.

Explanation:

Hello,

On the attached picture you will find the chemical reaction forming the required product, 4-chloro-4-methyl-cyclohexene. In this case, according to the Markovnicov’s rule, it is more likely for the chlorine to be substituted at the carbon containing the methyl radical in addition to the hydrogen to the next carbon to break the double bond and yield the presented product.

Best regards.

The dienes are the compounds comprised of two double bonds in the structure. The reaction of sodium phenoxide with HCl produced phenol and the salt.

The substitution reaction is defined as the reaction in which the element is substituted or replaced by the reactive other element.

In diene molecules, the double bonds add the partial charge to the compound, and  the HCl or the other reactant in the product is diverted to join at the double bonds in the diene.

The image attached is the reaction of sodium phenoxide with the HCl. The reaction carried the process of substitution of H at the place of  Na, with the formation of phenol.

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Answer: 20%

Explanation:

Relative error = Absolute error/actual value

= 0.1/0.5

= 0.2

Hence,

Minimum % Relative error = 0.2 ×100%

= 20%

Answer:20%

Explanation:

Let us take some important definitions of some terms in the question.

What is an ABSOLUTE ERROR?.

Absolute error is the difference between the expected value and the value you got from an experimental calculations or the approximations made. It can be represented mathematically in the equation (1) below;

Absolute error= expected value - Approximated/measured value. ---------------------------------------------------------------------(1).

What is A RELATIVE ERROR?.

A relative error is the the ratio of absolute value to that of the exact value. This can be illustrated mathematically by the equation (2) below;

Relative error= absolute error/exact value. --------------------------------------(3).

From equation (2) the solutio to the question is;

Relative error= absolute error/exact value.

Relative error=[ 0.1/0.5] = 0.2.

Relative error Percentage= 0.2×100= 20 Percent.

Answer: The millimoles of sodium carbonate the chemist has added to the flask are 256

Explanation:

Molarity is defined as the number of moles dissolved per liter of the solution.

To calculate the number of moles for given molarity, we use the equation:

[tex]\text{Molarity of the solution}=\frac{\text{milli moles of solute}}{\text{Volume of solution in ml}}[/tex]     .....(1)

Molarity of [tex]BaCl_2[/tex] solution = 1.42 M

Volume of solution = 180.0 mL

Putting values in equation 1, we get:

[tex]1.42M=\frac{\text{milli moles of }BaCl_2}{180.0ml}\\\\\text{milli moles of }BaCl_2}={1.42M\times 180.0ml}=256milli mol[/tex]

Thus the millimoles of sodium carbonate the chemist has added to the flask are 256.

In order to calculate the millimoles of sodium carbonate added to the flask, one must rearrange the formula for molarity, convert the volume from milliliters to liters, substitute, solve, then, finally, convert the solution from moles to millimoles. This results in an approximate 255.6mmol of sodium carbonate.

The chemist added 180.0 mL of a 1.42M sodium carbonate (Na2CO3) solution. Molarity (M) is defined as the number of moles of solute (Na2CO3 in this case) per liter of solution. Therefore, to find the number of millimoles, you would use the equation:

M = moles/volume(L)

Rearrange the formula to solve for moles:

moles = M x volume (L)

Next, convert the volume from milliliters to liters: 180.0 mL = 0.180 L. Substituting into the equation gives:

moles = 1.42M x 0.180 L = 0.2556 moles

To convert moles to millimoles, you'll need to know that 1 mole = 1000 millimoles. Therefore, 0.2556 moles x 1000 = 255.6 millimoles rounded to three significant digits.

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Answer: It will occupy [tex]4.45\times 10^3ml[/tex] at the same temperature and 475 mm Hg.

Explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

[tex]P\propto \frac{1}{V}[/tex]     (At constant temperature and number of moles)

[tex]P_1V_1=P_2V_2[/tex]    (At constant temperature and number of moles)

where,

[tex]P_1[/tex] = initial pressure of gas = 760 mm Hg

[tex]P_2[/tex] = final pressure of gas = 475 mm Hg

[tex]V_1[/tex] = initial volume of gas = [tex]2.78\times 10^3ml[/tex]

[tex]V_2[/tex]  = final volume of gas = ?

Putting in the values:

[tex]760mm Hg\times 2.78\times 10^3ml=475 mm Hg\times V_2[/tex]

[tex]V_2=4.45\times 10^3ml[/tex]

Thus it will occupy [tex]4.45\times 10^3ml[/tex] at the same temperature and 475 mm Hg

The volume that it will occupy at the same temperature is 4448mL

According to Boyle's law, the pressure of a given mass of gas is inversely proportional to the volume. It is expressed mathematically as:

[tex]P\alpha\frac{1}{V}\\P=\frac{k}{V}\\PV=k[/tex]

This can be expressed as [tex]P_1V_1=P_2V_2[/tex]

Given the following parameters

P₁ = 760mmHg

V₁ = 2.78 x 10³ mL

P₂ = 475mmHg

V₂ = ?

Substitute the given parameters into the formula

[tex]V_2=\frac{P_1V_1}{P_2}\\V_2=\frac{760\times 2780}{475}\\V_2= 4448mL[/tex]

Hence the volume that it will occupy at the same temperature is 4448mL

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Answer: option B. there are 35 mg of lead in 1.0 L of this solution

Explanation:

1ppm = 1mg/L

Therefore 35ppm = 35mg/L

So, the solution contains 35mg of lead in 1L of the solution

Answer:

79.0 mL

Explanation:

Given data

In order to find the volume required of the concentrated solution, we will use the dilution rule.

C₁ × V₁ = C₂ × V₂

V₁ = C₂ × V₂/C₁

V₁ = 1.00 M × 790.0 mL/10.0 M

V₁ = 79.0 mL

Answer: [tex]2NaOH(aq)+MgCl_2(aq)\rightarrow NaCl(aq)+Mg(OH)_2(s)[/tex]

Explanation:

According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.

A double displacement reaction is one in which exchange of ions take place. The salts which are soluble in water are designated by symbol (aq) and those which are insoluble in water and remain in solid form are represented by (s) after their chemical formulas.

[tex]2NaOH(aq)+MgCl_2(aq)\rightarrow NaCl(aq)+Mg(OH)_2(s)[/tex]