Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
Question
Chapter 11, Problem 52SCQ

(a)

Interpretation Introduction

Interpretation:

The reason for H2S being a gas at normal pressure and water being a liquid has to be determined.

Concept Introduction:

  • Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
  • Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
  • Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

    xa=nantotal

  • pa=xa×Ptotal

    Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

(a)

Expert Solution
Check Mark

Explanation of Solution

The major reason behind this observation is hydrogen bonding The electronegativity difference between hydrogen and oxygen is very large. So the intermolecular force of attraction is high. But the electronegativity difference between hydrogen and sulphur is comparatively low.

Comparing H2S and water , energy required to overcome the forces of attraction is less for H2S than water. This energy can be easily taken from room temperature.

Thus H2S exist as a gas and water exist as a liquid at room temperature.

(b)

Interpretation Introduction

Interpretation:

The partial pressure of H2S has to determined.

Concept Introduction:

  • Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
  • Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
  • Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

    xa=nantotal

  • pa=xa×Ptotal

    Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

(b)

Expert Solution
Check Mark

Explanation of Solution

The partial pressure of H2S at given conditions.

Given:

ConcentrationofH2S=80ppmV=1LPTotal=725mmHg

M=ppmMolecularmass×1000

Molarity of H2S=8034.08×1000=2.347×10-3mol/L

Numberofmoles=Molarity×VolumeNumberofmolesofH2S=2.347×10-3×1=2.347×10-3moles

Using the given data we can find out the total number of moles in the mixture.

PV=nRT

n=PVRT=0.9539×10.0831×295=0.039166moles

MolefractionofH2S=2.347×10-3moles0.039166moles=0.0599

pa=xa×PtotalpH2S=0.05992×0.9539=0.0571atm

(c)

Interpretation Introduction

Interpretation:

The amount of oxygen required to convert the given amount of H2S to H2SO4 has to be given.

Concept Introduction:

  • Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
  • Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
  • Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

    xa=nantotal

  • pa=xa×Ptotal

    Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

(c)

Expert Solution
Check Mark

Explanation of Solution

Given:

H2S+2O2H2SO4

VolumeofH2S=5.2LP=130mmHg=0.1710atmT=25°C=298K

Using ideal gas equation we can calculate the number of moles of H2S

n=PVRT=0.1710×5.20.0829×298=0.036moles

From the balanced equation it is clear that if one mole of H2S react with 2 moles of O2 , we will get one mole of H2SO4

Number of moles of O2 required to complete the reaction will be 0.072molesO2(0.036×2)

Using the ideal gas equation we can calculate the volume of oxygen needed to complete the reaction.

PV=nRT

V=nRTP=0.072×0.0829×2980.1710=10.4L

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Chemistry & Chemical Reactivity

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