   Chapter 15, Problem 56GQ

Chapter
Section
Textbook Problem

Sulfuryl chloride, SO2Cl2 is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to SO2 and Cl2.SO2Cl2(g) ⇄ SO2(g) + Cl2(g)    Kc = 0.045 at 375 °C (a) A 10.0-L flask containing 6.70 g of SO2Cl2 is heated to 375 °C. What is the concentration of each of the compounds in the system when equilibrium is achieved? What fraction of SO2Cl2 has dissociated? (b) What are the concentrations of SO2Cl2, SO2, and Cl2 at equilibrium in the 10.0-L flask at 375 °C if you begin with a mixture of SO2Cl2 (6.70 g) and Cl2 (0.10 atm)? What fraction of SO2Cl2 has dissociated? (c) Compare the fractions of SO2Cl2 in parts (a) and (b). Do they agree with your expectations based on Le Chatelier’s principle?

(a)

Interpretation Introduction

Interpretation:

The concentration of the compounds in the decomposition of SO2Cl2 at equilibrium and the fraction of SO2Cl2 that has dissociated has to be identified.

Concept Introduction:

Equilibrium constant in terms of concentrationKC:

aA(g)+bB(g)cC(g)+dD(g)KC=[C]c×[D]d[A]a×[B]b

Molarity=NumberofmolesVolumeofsolution(L)

Idealgasequation:PV=nRT

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Like wise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Explanation

Given:

SO2Cl2(g)SO2(g)+Cl2(g)KC=0.045MassofSO2Cl2=6.70gT=375°C=648KV=10L

nSO2Cl2=massofSO2Cl2Molarmass=6.7g135g/mol=0.0496mol

SO2Cl2(g)SO2(g)+Cl2(g)Initial0.0496300Changex+x+xEquilibrium0

(b)

Interpretation Introduction

Interpretation:

The concentration of the compounds in the decomposition of SO2Cl2 at equilibrium and the fraction of SO2Cl2 that has dissociated has to be identified.

Concept Introduction:

Equilibrium constant in terms of concentrationKC:

aA(g)+bB(g)cC(g)+dD(g)KC=[C]c×[D]d[A]a×[B]b

Molarity=NumberofmolesVolumeofsolution(L)

Idealgasequation:PV=nRT

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

Interpretation Introduction

Interpretation:

The fraction of SO2Cl2 that has dissociated has to be compared.

Concept Introduction:

Le Chatelier’s principle: If equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.

Factor’s that effect chemical equilibria:

Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Like wise adding products increase yield of reactants.

Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.

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