Explain the effect of the following stresses on the position of the equilibrium

Question

Explain the effect of the following stresses on the position of the equilibrium

SO3(g) SO2(g) + 1 2 O2(g)

The reaction as written is endothermic.

(a) O2(g) is added to the equilibrium mixture without changing volume or temperature.

(b) The mixture is compressed at constant temperature.

(c) The equilibrium mixture is cooled.

(d) An inert gas is pumped into the equilibrium mixture while the total gas pressure and the temperature are kept constant.

(e) An inert gas is added to the equilibrium mixture without changing the volume. (f) SO2(g) is removed from the system.

Explanation / Answer

SO3(g) ? SO2(g) + 1/2 O2(g) delta H = positive.

Following the Le Chatelier's Principles,

(a) adding oxygen favours the reverse reaction, that is, formation of SO3

(b) Since all the reagents in the reaction is gas, compressing the mixture at constant temperature, decreases the volume and hence the reverse reaction, that is, formation of SO3 is favoured

(c) Since the rection is endothermic, cooling the temperature favours reversible reaction,  that is, formation of SO3

(d) adding inert gas to mixture occupies some space, therefore again formation of SO3 is favoured

(e) adding inert gas at constant volume increases the pressure and temperature, therefore, decomposition of SO3 is favoured

(e) removing SO2(g) favours the forward reaction, that is, formation of oxygen.

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