Ncert Exercises & Solutions

On the basis of Le-Chatelier principle explain how temperature and pressure can be adjusted to increase the yield of ammonia in the following reaction.

$N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g); ∆ H = - 92.38 kJ {mol}^{- 1}$

What will be the effect of addition of argon to the above reaction mixture at constant volume?

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g); ∆ H = - 92.38 kJ {mol}^{- 1}

It is an exothermic process as

∆ H

is negative.

Effect of temperature According to Le-Chatelier's principle, low temperature is favourable for high yield of ammonia, but practically very low temperatures slow down the reaction. So, optimum temperature 700 K is favourable in attainment of equilibrium.

Effect of pressure Similarly, high pressure about 200 atm is favourable for high yield of ammonia. On increasing pressure, reaction goes in the forward direction because the number of moles decreases in the forward direction.

Addition of argon At constant volume addition of argon does not affect the equilibrium because it does not change the partial pressures of the reactants or products involved in the reaction and the equilibrium remains undisturbed.

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