Reaction quotient for the reaction, N2( g)+3 H2( g) ⇄2 NH3( g) is given by Q=([NH3]^2)/([ N2][H2

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Reaction quotient for the reaction, N2( g)+3 H2( g) ⇄2...

Reaction quotient for the reaction, $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftarrows 2 \mathrm{NH}_3(\mathrm{~g})$ is given by $\mathrm{Q}=\frac{\left[\mathrm{NH}_3\right]^2}{\left[\mathrm{~N}_2\right]\left[\mathrm{H}_2\right]^3}$ the reaction will proceed from right to left, if $\mathrm{K}_{\mathrm{c}}$ is equilibrium constant (a) $\mathrm{Q}<\mathrm{K}_{\mathrm{c}}$ (b) $\mathrm{Q}=0$ (c) $\mathrm{Q}>\mathrm{K}_{\mathrm{c}}$ (d) $\mathrm{Q}=\mathrm{K}_{\text {}}$

Reaction quotient for the reaction, $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftarrows 2 \mathrm{NH}_3(\mathrm{~g})$ is given by $\mathrm{Q}=\frac{\left[\mathrm{NH}_3\right]^2}{\left[\mathrm{~N}_2\right]\left[\mathrm{H}_2\right]^3}$
the reaction will proceed from right to left, if $\mathrm{K}_{\mathrm{c}}$ is equilibrium constant
(a) $\mathrm{Q}<\mathrm{K}_{\mathrm{c}}$
(b) $\mathrm{Q}=0$
(c) $\mathrm{Q}>\mathrm{K}_{\mathrm{c}}$
(d) $\mathrm{Q}=\mathrm{K}_{\text {}}$

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Key Concepts

Reaction Shift Based on Q and K

By comparing the reaction quotient (Q) to the equilibrium constant (K), one can predict the direction in which a reaction will proceed to reach equilibrium. Specifically, if Q is greater than K, the reaction will shift to the left (toward the reactants) to achieve equilibrium, and if Q is less than K, it will shift to the right (toward the products).

Reaction Quotient

The reaction quotient is an expression that represents the ratio of the concentrations or pressures of the reaction’s products to those of its reactants, each raised to the power of their stoichiometric coefficients. It is used to gauge the current state of a reaction in relation to equilibrium.

Equilibrium Constant

The equilibrium constant is a fixed value at a given temperature that expresses the ratio of the concentrations or pressures of the products to those of the reactants when the reaction is at equilibrium. It is derived from the law of mass action and represents the balance point of the reaction.

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