Question

In: Chemistry

1. Predict whether each of the following equilibria will shift toward products or reactants with a...

1. Predict whether each of the following equilibria will shift toward products or reactants with a temperature increase:

a. CH4(g) + H2O(g) === CO(g) + 3H2( g) Delta H = +206kJ

b. CO(g) + H2O(g) CO2(g) + H2(g) Delta H = -41 kJ

c. 2SO2(g) + O2(g) = 2SO3(g) Delta H = -198 kJ

d. N2O4 (g) ===== 2NO2 (g) Delta H = + 57kJ

Expert Solution

1. a. when increasing temperature of the given reaction, the equilibrium will shift towards products.

CH4(g) + H2O(g) <===> CO(g) + 3H2( g) ΔH = +206kJ

The above reaction is endothermic because ΔH is positive, thus reaction favours the formation of products at higher temperature. Therefore, the position of equilibrium shifts to the right side.

b. when increasing temperature of the given reaction, the equilibrium will shift towards reactants

CO(g) + H2O(g) <====> CO2(g) + H2(g) ΔH = -41 kJ

The above reaction is exothermic because ΔH is negative, thus reaction favours the formation of reactants at higher temperature. Therefore, the position of equilibrium shifts to the left side.

c. when increasing temperature of the given reaction, the equilibrium will shift towards reactants

2SO2(g) + O2(g) <===> 2SO3(g) Δ H = -198 kJ

The above reaction is exothermic because ΔH is negative, thus reaction favours the formation of reactants at higher temperature. Therefore, the position of equilibrium shifts to the left side.

d. when increasing temperature of the given reaction, the equilibrium will shift towards products.

N2O4 (g) <====> 2NO2 (g) Δ H = + 57kJ

The above reaction is endothermic because ΔH is positive, thus reaction favours the formation of products at higher temperature. Therefore, the position of equilibrium shifts to the right side.

queen_honey_blossom answered 1 year ago

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