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

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.

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

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

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)

ΔH = 92kJ  Endothermic reaction

Equilibrium will shift in right that is the forward direction.

On decrease in volume:

Equilibrium will shift in left that is the backward direction.

(b)

ΔH =181kJ  Endothermic reaction

Equilibrium will shift in right that is the forward direction.

On decrease in volume:

Equilibrium will shift in right that is the forward direction.

(c)

ΔH = − 285kJ  Exothermic reaction

Equilibrium will shift in right that is the forward direction.

On decrease in volume:

Equilibrium will shift in left that is the backward direction.

(d)

ΔH = − 176kJ Exothermic reaction

Equilibrium will shift in right that is the forward direction.

On decrease in volume:

Equilibrium will shift in right that is the forward direction.

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explanation: no but i do not usually comment