${{\mathrm{I}}_{2}}_{\left(\mathrm{s}\right)}$ $+$ $5{{\mathrm{F}}_{2}}_{\left(\mathrm{g}\right)}$  $\to 2{\mathrm{IF}}_{5\left(g\right)}$ 

The equilibrium constant Kc expression for the above mentioned reaction is:
 1 $$\mathrm{K_{C} = \dfrac{\left[IF_{5}\right]^{2}}{\left[F_{2}\right]^{5}}}$$ 2 $$\mathrm{K_{C} = \dfrac{\left[IF_{5}\right]^{2}}{\left[F_{2}\right]^{5} \left[I_{2}\right]}}$$ 3 $$\mathrm{K_{C} = \dfrac{\left[F_{2}\right]^{5} \left[I_{2}\right]}{\left[IF_{2}\right]^{2}}}$$ 4 $$\mathrm{K_{C} = \dfrac{\left[F_{2}\right]^{5}}{\left[IF_{5}\right]^{2}}}$$
Subtopic:  Introduction To Equilibrium |
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${\mathrm{K}}_{{\mathrm{a}}_{1}},$ ${\mathrm{K}}_{{\mathrm{a}}_{2}}$ $\mathrm{and}$ ${\mathrm{K}}_{{\mathrm{a}}_{3}}$ are the respective ionisation constants for the following reactions.
$$\mathrm{H}_2 \mathrm{~S} \rightleftharpoons \mathrm{H}^{+}+\mathrm{HS}^{-}$$
$$\mathrm{HS}^{-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{S}^{2-}$$
$$\mathrm{H}_2 \mathrm{~S} \rightleftharpoons 2 \mathrm{H}^{+}+\mathrm{S}^{2-}$$
The correct relationship between ${\mathrm{K}}_{{\mathrm{a}}_{1}},$ ${\mathrm{K}}_{{\mathrm{a}}_{2}}$ $\mathrm{and}$ ${\mathrm{K}}_{{\mathrm{a}}_{3}}$ is:
1. $$\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} \times \mathrm{K}_{\mathrm{a}_2}$$
2. $$\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1}+\mathrm{K}_{\mathrm{a}_2}$$
3. $$K_{a_3}=K_{a_1}-K_{a_2}$$
4. $$\mathrm{K}_{\mathrm{a}_3}=\mathrm{K}_{\mathrm{a}_1} / \mathrm{K}_{\mathrm{a}_2}$$

Subtopic:  Introduction To Equilibrium |
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Reaction quotient for the reaction, ${\mathrm{N}}_{2}\left(\mathrm{g}\right)+3{\mathrm{H}}_{2}\left(\mathrm{g}\right)⇌2{\mathrm{NH}}_{3}\left(\mathrm{g}\right)$ 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 Kc value is:

 1 QKc 4 Q=Kc
Subtopic:  Introduction To Equilibrium |
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In the reaction A(g) + 2B(g) ⇌ 2C(g) + D(g), the initial concentration of B is twice that of A and, at equilibrium, the concentrations of A and D are equal. The value of the equilibrium constant will be:

 1 4 2 16 3 2 4 1
Subtopic:  Introduction To Equilibrium |
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