A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? $3H_2(g) + N_2(g) ightleftharpoons 2NH_3(g)$ More ammonia will be produced at the expense of hydrogen and nitrogen. There will be no effect. Hydrogen and nitrogen will be produced at the expense of ammonia. The equilibrium constant will increase. The equilibrium constant will decrease.
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Ronald P.
A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. If the volume of the container is increased at constant temperature, the equilibrium constant will increase: 3H2(g) + N2(g) → 2NH3(g)
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Ammonia is added to a gaseous reaction mixture containing $\mathrm{H}_{2}, \mathrm{Cl}_{2},$ and $\mathrm{HCl}$ that is at chemical equilibrium. How will the addition of ammonia affect the relative concentrations of $\mathrm{H}_{2}, \mathrm{Cl}_{2},$ and $\mathrm{HCl}$ if the equilibrium constant of reaction 2 is much greater than the equilibrium constant of reaction $1 ?$ (1) $\quad \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{HCl}(g)$ (2) $\quad \mathrm{HCl}(g)+\mathrm{NH}_{3}(g) \rightleftharpoons \mathrm{NH}_{4} \mathrm{Cl}(s)$
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