Question

URGENT

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

Step-by-step explanation:

Discussion

When Pressure increases equilibrium shifts to the side with the smallest number of moles. But which side is that?

N2(g) + 3H2(g) ⇌ 2NH3(g)

The left side has 1 mol of nitrogen (N2) and 3 moles of Hydrogen = 4 mols

on the left side.

The right side has 2 mols of NH3 = 2 mols on the right.

Conclusion: You tell the number of mols by the Balance numbers to the left of each chemical in an equation.

Since the left side N2 + 3H2 = 4 mols, the equilibrium does NOT shift left.

2NH3 is only two mols.

The equilibrium shifts Right

Answer

D