Le Châtelier's Principle and Concentration

Question

Consider the Haber process at equilibrium: $$\mathrm{N_2(g)} + 3\mathrm{H_2(g)} \rightleftharpoons 2\mathrm{NH_3(g)}$$. The table shows the concentrations of the species before and immediately after the concentration of $$\mathrm{H_2}$$ is increased at a constant temperature. Which of the following describes how the system will respond to reestablish equilibrium?

| Species | Initial Concentration (M) | After H2 Addition (M) |
|---------|-----------------------------|-----------------------|
| N2      | 0.5                         | 0.5                   |
| H2      | 1.5                         | 2.5                   |
| NH3     | 1.0                         | 1.0                   |

Accepted Answer

The equilibrium shifts to the right to produce more $$\mathrm{NH_3}$$.

Answer

The increased concentration of $$\mathrm{H_2}$$ has no effect on the reaction rates.

Answer

There is no shift in the equilibrium position.

Answer

The equilibrium shifts to the left to produce more $$\mathrm{N_2}$$ and $$\mathrm{H_2}$$.

Le Châtelier's Principle and Concentration

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