Question

1. The following equilibrium may be established with carbon dioxide and steam. CO(g) + H2O(g) ↔ CO2(g) + H2(g) ΔH = -41.12 kJ What would be the effect of each of the following on the equilibrium and concentrations?

a.) The addition of more H2O?

b.) The removal of some H2?

c.) Raising the temperature?

d.) Increasing the pressure?

e.) Addition of a catalyst?

Answer 1

CO(g) + H2O(g) ↔ CO2(g) + H2(g) ΔH = -41.12 kJ

a.) The addition of more H2O

When conc of reactants increases or conc of products decreases reaction favor fro ward direction

The addition of H2O conc of reactants are increases .So reaction shit for ward direction(right side)

b.) The removal of some H2

When conc of reactants increases or conc of products decreases reaction favor fro ward direction.

The removal of H2 conc of products are decreases So reactio shit for ward direction (right side)

c.) Raising the temperature.

At lower temperature exothermic reaction is takes place. At higher temperature edothermic reaction is takes place.

O(g) + H2O(g) ↔ CO2(g) + H2(g) ΔH = -41.12 kJ this reactio is exothermic reaction .So for ward reaction takes place at lower temp.

Temperature is increases back ward reaction is talesplace.Raising the temperature back ward reaction takes place.

d.) Increasing the pressure.

When pressure increases no of moles or volume decreases side reaction favorable.

The above reaction no pressure effect because of no of mole of reactants and no of moles of products are equal.

e.) Addition of a catalyst

Catalyst increases the rate far ward of reaction and rate of back ward reaction.