For the equilibrium reaction 2NH3 (g) + 22 kJ ↔ N2 (g) + 3H2 (g), which of the following changes would result in the formation of more N2 and H2 at equilibrium?

Question

Chemistry

Lauren Bradley

12 January, 04:18

For the equilibrium reaction 2NH3 (g) + 22 kJ ↔ N2 (g) + 3H2 (g), which of the following changes would result in the formation of more N2 and H2 at equilibrium?

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Answers (1)

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Jaqueline Mcbride · Answer 1

Hello! Your question seems incomplete, still I will try to answer it in a general way. As shown in in equation 22 KJ heat is absorbed during the reaction so it is endothermic reaction.

Effect of Temperature:

According to Le Chatelier's principle, by increasing temperature the equilibrium will shift in the forward direction hence more nitrogen and hydrogen will produce.

Effect of Pressure:

It is evident from the reaction that there is an increase in volume in the formation of N2 and H2 (4 moles in whole), Hence, decrease in pressure on this system in equilibrium state will adjust itself in a direction in which the volume is increased i. e. formation of N2 and H2.

Effect of Concentration:

Increasing concentration of NH3, removal of N2 or removal of H2 will shift the equilibrium in forward direction, Hence more product is formed.