Question

Consider the following equilibrium for the exothermic reaction: 2NaHSO3(s) <=> Na2SO3(s) +H2O(g) +SO2(g)

How will the equilibrium shift when each of the following changes are made separately? Answer with shift towards products, shift towards reactants or no shift. Provide a reason for your choice.

a.) Adding H2O to the reaction vessel:

b.) Adding Helium to the reaction vessel:

c.) Removing Na2SO3:

d.) Increasing the volume of the reaction vessel:

e.) Increasing the temperature of the reaction vessel:

Answer 1

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Adding H2O to the reaction vessel: when any of the product is added to an equilibrium, the equilibrium shifts in a direction where it can consume it. Thus, Adding H2O to the reaction vessel shifts the equilibrium to left.

Removing Na2SO3: removing any of the product in an equilibrium, th eequilibrium shiftd in a direction where it can replenish the loss. Thus, removing Na2SO3 shifts the equilibrium to left.

Increasing the volume of the reaction vessel: When volume increases pressure decreases and equlibrium shifts in a direction where there is morenumber of moles. In the given equilibrium number of moles of reactant (2 moles) is less than that of product (2 moles), thus, Increasing the volume of the reaction vessel shifts the equilibrium to right.

Increasing the temperature of the reaction vessel: An exothermic reaction indicates release of heat. Thus, Increasing the temperature of the reaction vessel of an exothermic reation shifts to left (since the towards left the reaction will be endothermic)