Suppose the following exothermic reaction is allowed to reach equilibrium. A(g)
ID: 716537 • Letter: S
Question
Suppose the following exothermic reaction is allowed to reach equilibrium.
A(g) + 3 B(g) 2 C(g) + 3 D(g)
Then we make each of the following changes and allow the reaction to reestablish equilibrium. Tell whether the amount of B present at the new equilibrium will be (1) greater than, (2) less than, or (3) the same as the amount of B before the change was imposed.
A. the temperature is decreased while the volume is kept constant. [ Select ] ["B is less than", "B is the same", "B is great than"]
B. more A is added [ Select ] ["B is greater than", "B is the same", "B is less than"]
C. more C is added [ Select ] ["B is greater than", "B is less than", "B is the same"]
D. a small amount of D is removed [ Select ] ["B is the same", "B is less than", "B is greater than"]
E. the pressure is increased by decreasing the volume [ Select ] ["B is greater than", "B is less than", "B is the same"]
Explanation / Answer
This can be explained by le-Chatelier principle.If we change the external parameters which determine the equilibrium of the system the reaction will orient itself in such a way that effect of this be minimized.This is known as Le-Chatelier principle.According to Vant hoff reaction isotherm here reaction quotient is
Q= aC2 × aD3/ a1A × a3B .Now
A. If temperature is decreased while the vol. Is kept constant then delta H will be greater than 0. Thats why forward reaction takes place. So B will be lesser here
B. If we add more A then Reaction quotient Q will be less than 0. To make it =0 forward reaction will be favoured. So B will be lesser here
C. If more C is added then then backward reaction will be favourerd and amount of B will be greater.
D. If small amount of D is removed the amount of "Q" will be less than previous. To make it same as previous forward reaction takes place and amount of B will be lesser.
E. If pressure is increased then backward reaction will be favoured and amount B will be greater.
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