Match the following equilibria with the corresponding condition.

 A. Liquid$⇌$Vapour 1 Saturated solution B. Solid$⇌$Liquid 2 Boiling point C. Solid$⇌$Vapour 3 Sublimation point D. Solute (s)$⇌$Solute (solution) 4 Melting point 5 Unsaturated solution

Codes:

 A B C D 1. 2 4 3 1 2. 1 2 3 5 3. 5 4 3 2 4. 4 5 3 2
Subtopic:  Introduction To Equilibrium |
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In the reaction, N2O4(g) $⇌$ 2NO2(g), $\mathrm{\alpha }$ is that part of N2O4 which dissociates. The number of moles at equilibrium will be:

1. ${\left(1-\mathrm{\alpha }\right)}^{2}$

2. $3\mathrm{\alpha }$

3. $\mathrm{\alpha }$

4. $1+\mathrm{\alpha }$

Subtopic:  Introduction To Equilibrium |
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${{\mathrm{I}}_{2}}_{\left(\mathrm{s}\right)}$ $+$ $5{{\mathrm{F}}_{2}}_{\left(\mathrm{g}\right)}$  $\to 2{\mathrm{IF}}_{5\left(g\right)}$ 

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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If the molar concentration of ${\mathrm{SnCl}}_{4}$ is $1.5$ $×$ ${10}^{-3}$ mol L–1, the concentration of chloride ions will be:

 1 3.0 x 10-3 2 6.0 x 10-3 3 0.3 x 10-3 4 0.6 x 10-6
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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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An incorrect statement about equilibrium among the following is:

 1 Equilibrium is possible only in a closed system at a constant temperature. 2 All measurable properties of the system remain constant. 3 All the physical processes stop at equilibrium. 4 The opposing processes occur at the same rate and there is a dynamic but stable condition.
Subtopic:  Introduction To Equilibrium |
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For a reaction, 2NO (g) + Br2 (g)  $⇋$2NOBr (g)

When 0.087 mol of NO and 0.0437 mol of Br2 are mixed in a closed container at a constant temperature, 0.0518 mol of NOBr is obtained at equilibrium. The concentration of NO and Br2 at equilibrium will be:

1. NO = 0.0352 mol; ${\mathrm{Br}}_{2}$= 0.0178 mol

2. NO = 0.352 mol; ${\mathrm{Br}}_{2}$= 0.178 mol

3. NO = 0.0634 mol; ${\mathrm{Br}}_{2}$= 0.0596 mol

4. NO = 0.634 mol; ${\mathrm{Br}}_{2}$= 0.596 mol

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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
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Which of the following is an example of a reversible reaction?

 1 $$\small{KNO_3(aq) + NaCl(aq) \rightleftharpoons KCl(aq) + NaNO_3(aq)}$$ 2 $$\small{2Na(s) + H_2O(l) \rightleftharpoons 2NaOH(aq) + H_2(g)}$$ 3 $$\small{AgNO_3(aq) + NaCl(aq) \rightleftharpoons AgCl(s) + NaNO_3(aq)}$$ 4 $$\small{Pb{(NO_3)}_2(aq) + 2NaI(aq) \rightleftharpoons PbI_2(s) + 2NaNO_3(aq)}$$
Subtopic:  Introduction To Equilibrium |
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