$N_2 + 3 H_2 \rightleftharpoons 2 NH_3$
Which statement is correct if $N_2$ is added at equilibrium condition?
Which statement is correct if $N_2$ is added at equilibrium condition?
- AThe equilibrium will shift to the forward direction because according to the $II^{nd}$ law of thermodynamics,the entropy must increase in the direction of a spontaneous reaction.
- BThe condition for equilibrium is $G_{N_2} + 3 G_{H_2} = 2 G_{NH_3}$,where $G$ is the Gibbs free energy per mole of the gaseous species measured at that partial pressure. The condition of equilibrium is unaffected by the use of a catalyst,which increases the rate of both the forward and backward reactions to the same extent.
- CThe catalyst will increase the rate of the forward reaction by $\alpha$ and that of the backward reaction by $\beta$.
- D$A$ catalyst will not alter the rate of either reaction.
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Similar Questions
The following reaction occurs in the blast furnace where iron ore is reduced to iron metal:
$Fe_2O_{3(s)} + 3CO_{(g)} \rightleftharpoons 2Fe_{(l)} + 3CO_{2(g)}$
Using Le Chatelier's principle,predict which one of the following will not disturb the equilibrium.
$Fe_2O_{3(s)} + 3CO_{(g)} \rightleftharpoons 2Fe_{(l)} + 3CO_{2(g)}$
Using Le Chatelier's principle,predict which one of the following will not disturb the equilibrium.
In the reaction $A_{(g)} + 2B_{(g)} \rightleftharpoons C_{(g)} + Q \ kJ$,greater product will be obtained or the forward reaction is favoured by:
Medium
View SolutionWhich of the following reactions will be affected by increasing the pressure? Also,mention whether the change will cause the reaction to proceed in the forward or backward direction.
$(i)$ $CaCl_{2(s)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$
$(ii)$ $CH_{4(g)} + 2S_{2(g)} \rightleftharpoons CS_{2(g)} + 2H_{2}S_{(g)}$
$(iii)$ $CO_{2(g)} \rightleftharpoons C_{(s)} + 2CO_{(g)}$
$(iv)$ $2H_{2(g)} + CO_{(g)} \rightleftharpoons CH_{3}OH_{(g)}$
$(v)$ $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$
$(vi)$ $4NH_{3(g)} + 5O_{2(g)} \rightleftharpoons 4NO_{(g)} + 6H_{2}O_{(g)}$
$(i)$ $CaCl_{2(s)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$
$(ii)$ $CH_{4(g)} + 2S_{2(g)} \rightleftharpoons CS_{2(g)} + 2H_{2}S_{(g)}$
$(iii)$ $CO_{2(g)} \rightleftharpoons C_{(s)} + 2CO_{(g)}$
$(iv)$ $2H_{2(g)} + CO_{(g)} \rightleftharpoons CH_{3}OH_{(g)}$
$(v)$ $CaCO_{3(s)} \rightleftharpoons CaO_{(s)} + CO_{2(g)}$
$(vi)$ $4NH_{3(g)} + 5O_{2(g)} \rightleftharpoons 4NO_{(g)} + 6H_{2}O_{(g)}$
Difficult
View SolutionIn which of the following reactions will an increase in pressure lead to an increase in the yield of products?
Medium
View Solution$2x_{(g)} + y_{(g)} \rightleftarrows 2z_{(g)} + 80 \ kcal$
Which combination gives the highest yield of $z$ at equilibrium?
Which combination gives the highest yield of $z$ at equilibrium?
Medium
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