Question

Given the equation representing a reaction at equilibrium:
N2(g) + 3H2(g) <==>2NH3(g)
What occurs when the concentration of H2(g) is increased?
(1) The equilibrium shifts to the left, and the concentration of N2(g) decreases.
(2) The equilibrium shifts to the left, and the concentration of N2(g) increases.
(3) The equilibrium shifts to the right, and the concentration of N2(g) decreases.
(4) The equilibrium shifts to the right, and the concentration of N2(g) increases.

Answer 1

Your answer would be 3) The equilibrium shifts to the right, and the concentration of N2 (g) decreases.

Answer 2

Looking at the reaction in equilibrium, an increase in the concentration of H2 will make the equilibrium shift to the right with an increase in the concentration of NH3.

Equilibrium reactions

When a reaction is in equilibrium and one of the constraints that affect the rate of reaction is applied, the equilibrium will shift to annul the effects created by the constraint.

H2 (g) is a reactant and when more reactant is added to a reaction in equilibrium, more of the products would be formed.

Thus, adding more H2 (g) will make the reaction shift to the right - towards the product. More N2 (g) will be consumed as a result.

More on equilibrium reactions can be found here: https://brainly.com/question/11114490