Question

Given that evaporation is an endothermic process, which of the following sets of changes would cause the following system at equilibrium to shift to increase the number of I₂ molecules in the gas phase? I₂(s) ⇌ I₂(g)

a. Increasing container volume and increasing temperature

b. Increasing container volume and decreasing temperature

c. Decreasing container volume and increasing temperature

d. Decreasing container volume and decreasing temperature

e. Changing volume or temperature will not affect the number of gas molecules present at equilibrium

Answer 1

I2(s) ---------------- I2(g)

n = number of moles of gaseous products - number of moles of gasous reactants

n = 1-0 =1

During the forword direction number of moles are increases.

when volume is increases , the equilibrium shifts towords to the number of moles increases side.

The Endothermic reactions are favoured at high temperatures.So the forword reactio is favoured at high temperature.

Hence, Increasing the container volume and increasing the temperature.

The answer is A.