Question

ASAP

A chemical 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

Answer 1

The chemical equilibrium is the state at which the rate of reaction is constant. The increase in pressure shifts the reaction towards the product side, as fewer moles of the product are there.

What are the factors affecting the chemical equilibrium?

The chemical equilibrium is shifters with the change in the concentration, temperature, pressure, and volume of the reaction.

The increase in the pressure results in more contact between the reactant molecules, as they are more in number and moles in the reaction.

The increased collision of the reactant molecules tried to reach the equilibrium condition, and the increased formation of the product is observed.

Thus, the increase in the pressure shifts the chemical equilibrium towards the product, as there were few moles of the product in the reaction.

Learn more about chemical equilibrium, here:

https://brainly.com/question/4289021

Answer 2

Answer:

its C

Explanation:

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