APFIVE Le Châtelier's Principle and Concentration
For the Haber process $$\mathrm{N_2(g)} + 3*\mathrm{H_2(g)} \rightleftharpoons 2*\mathrm{NH_3(g)}$$ illustrated in the table, how does the system respond when the concentration of $$\mathrm{H_2}$$ is increased while keeping the temperature constant?
| Species | Initial Concentration (M) | After H2 Addition (M) |
|---|---|---|
| N2 | 0.5 | 0.5 |
| H2 | 1.5 | 2.5 |
| NH3 | 1.0 | 1.0 |
A
The increased concentration of $$\mathrm{H_2}$$ has no effect on the reaction rates.
B
The equilibrium shifts to the right to produce more $$\mathrm{NH_3}$$.
C
The equilibrium shifts to the left to produce more $$\mathrm{N_2}$$ and $$\mathrm{H_2}$$.
D
There is no shift in the equilibrium position.
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