How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each?
(a) 2NH3(g) ⇌ N2(g)+3H2(g) ΔH = 92kJ

(b) N2(g) + O2(g) ⇌ 2NO(g) ΔH =181kJ

(c) 2O3(g) ⇌ 3O2(g) ΔH = − 285kJ

(d) CaO(s) + CO2(g) ⇌ CaCO3(s) ΔH = − 176kJ

Question

06-01-2020
Chemistry

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How will an increase in temperature affect each of the following equilibria? How will a decrease in the volume of the reaction vessel affect each?
(a) 2NH3(g) ⇌ N2(g)+3H2(g) ΔH = 92kJ

(b) N2(g) + O2(g) ⇌ 2NO(g) ΔH =181kJ

(c) 2O3(g) ⇌ 3O2(g) ΔH = − 285kJ

(d) CaO(s) + CO2(g) ⇌ CaCO3(s) ΔH = − 176kJ

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Tringa0 Tringa0 · Answer 1 · 2020-01-07T06:49:37+01:00

Explanation:

Any change in the equilibrium is studied on the basis of Le-Chatelier's principle. This principle states that if there is any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.

[tex]A\rightleftharpoons B+\text{ heat}[/tex]

In exothermic reaction , heat is released during a chemical reaction. This means that temperature is decreased on the reactant side.

Increasing temperature increase the heat on the product side, the equilibrium will shift in left direction.
Decreasing temperature decreases the heat on the product side, the equilibrium will shift in right direction.

[tex]A+\text{ heat}\rightleftharpoons B[/tex]

In endothermic reaction , heat is absorbed during a chemical reaction. This means that temperature is increased on the reactant side.

Increasing temperature increase the heat on the reactant side, the equilibrium will shift in right direction.
Decreasing temperature decreases the heat on the reactant side, the equilibrium will shift in left direction.

Increase the volume

If the volume of the container is decreased , the pressure will increase according to Boyle's Law. Now, according to the Le-Chatlier's principle, the equilibrium will shift in the direction where decrease in pressure is taking place. So the equilibrium will shift in direction where gaseous moles are less.

(a)[tex] 2NH_3(g)\rightleftharpoons N_2(g)+3H_2(g)[/tex]

ΔH = 92kJ Endothermic reaction