Given the gas-phase reaction 2SO_2(g) + O_2(g) 2SO_3(g). Suppose that the reacti

Question

Given the gas-phase reaction 2SO_2(g) + O_2(g) 2SO_3(g). Suppose that the reaction has already taken place, and the system has come to equilibrium. If the following changes are made to the system in equilibrium, tell what effect these changes with have on the system (whether the equilibrium is shifted to the left, is shifted to the right, or is not shifted). a. Additional O_2 is added to the system. ___ b. Sulfur trioxide is removed from the system as soon as it forms. ___ c. The pressure of the system is decreased (all components are gases). ___ d. A very efficient catalyst is used for the reaction. ___

Explanation / Answer

The reaction here is gaseous phase reversible one. Since at equilibrium the concentration of products and reactants doesn't anymore change with time and the rates of forward and backward reaction is same. Thus any change or stress caused on equilibrium position will make equilibrium to shift in such a way to balance the excess condition.

a. Increasing O2 concentration the equilibrium shifts to right. So as to reduce the concentration of reactant O2.

b. Removing Sulphur trioxide as soon as it forms will cause equilibrium to shift in such way so as to increase its concentration again, so it shifts Right.

c. As all components are gaseous and gas pressure is caused by collisions between gas molecules and reaction vessel. And concentrations are same only way to balance the pressure is to reduce moles of gases. As there are less moles on right, product side, equilibrium will shift to Right.

d. Using catalyst at equilibrium, as it speeds up both forward and backward reactions to same extent, there will be No shift in equilibrium.

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