Achemical equilibrium between gaseous reactants and products is shown. n2(g) + 3h2(g) ⇌ 2nh3(g) how will the reaction be affected if the pressure on the system is increased? it will shift toward the reactant side as there is lower pressure on the reactant side. it will shift toward the product side as there is higher pressure on the product side. it will shift toward the reactant side as there are a greater number of moles of gas on the reactant side. it will shift toward the product side as there are a fewer number of moles of gas on the product side.

Option (d) is the correct answer.

Explanation:

The given reaction is as follows.

When we increase the pressure then reactant molecules, that is, nitrogen and hydrogen gas will come closer to each other. As a result, there will be increase in formation of products. Therefore, rate of reaction will increase.

Also, according to LeChatelier's principle, there are more number of reactants  and hence, equilibrium will shift to the side where there is less stress, that is, on the product side.

Thus, we can conclude that it will shift toward the product side as there are a fewer number of moles of gas on the product side.

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