Problem 15.61 Consider the following equilibrium, for which H < 0 2SO2( g )+O2(
ID: 939497 • Letter: P
Question
Problem 15.61
Consider the following equilibrium, for which H< 0
2SO2(g)+O2(g)2SO3(g)
How will each of the following changes affect an equilibrium mixture of the three gases?
Part A
O2(g) is added to the system
is added to the system
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Part B
the reaction mixture is heated
the reaction mixture is heated
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Part C
the volume of the reaction vessel is doubled
the volume of the reaction vessel is doubled
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Part D
a catalyst is added to the mixture
a catalyst is added to the mixture
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Part E
the total pressure of the system is increased by adding a noble gas
the total pressure of the system is increased by adding a noble gas
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Part F
SO3(g) is removed from the system
is removed from the system
shift equilibrium to the right shift equilibrium to the left no affectExplanation / Answer
1 When oxygen is added, there is an increase in number of moles of reactants. This will shift the equilibrium so as to reduce the number of moles. So more SO3 formation takes place.
2. the reaction is exothermic. When the mixture is heated, the reaction moves so as to nullify the effect of increase in temperature. The reaction will have to proceed in the endothermic diretion
3. At constant temperature and pressure, volume is proportional to number of moles. As the volume increases, number of moles also increases and the reaction shifts to the right to compensat this ffect.
4. for oxidation of SO2 to SO3, V2O5 is the catalyst. Catalyst does not participate nor shift the equilibrium. It allows the reaction rate of forward and backward reactions to increase.
5. Noble gas does not have any effect on the equilibrium.
6.when SO3 is removed, there is reduction in number of moles of products. So to compensate this effect, the reaction proceeds in a direction where there is an increase in number of moles . The reaction shifts to the left.