Select Chapter Topics: 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 $⇌$ 2NO2$\mathrm{\alpha }$ 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 |
78%
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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:

$1.$ ${\mathrm{K}}_{\mathrm{C}}=$ $\frac{{\left[{\mathrm{IF}}_{5}\right]}^{2}}{{\left[{\mathrm{F}}_{2}\right]}^{5}}$
$2.$ ${\mathrm{K}}_{\mathrm{C}}=$ $\frac{{\left[{\mathrm{IF}}_{5}\right]}^{2}}{{\left[{\mathrm{F}}_{2}\right]}^{5}\left[{\mathrm{I}}_{2}\right]}$
$3.$ ${\mathrm{K}}_{\mathrm{C}}$ $=\frac{{\left[{\mathrm{F}}_{2}\right]}^{5}\left[{\mathrm{I}}_{2}\right]}{{\left[{\mathrm{IF}}_{2}\right]}^{2}}$
$4.$  ${\mathrm{K}}_{\mathrm{C}}$ $=\frac{{\left[{\mathrm{F}}_{2}\right]}^{5}}{{\left[{\mathrm{IF}}_{5}\right]}^{2}}$  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.

${\mathrm{H}}_{2}\mathrm{S}⇌{\mathrm{H}}^{+}+{\mathrm{HS}}^{-}$
${\mathrm{HS}}^{-}⇌{\mathrm{H}}^{+}+{\mathrm{S}}^{2-}$
${\mathrm{H}}_{2}\mathrm{S}⇌2{\mathrm{H}}^{+}+{\mathrm{S}}^{2-}$

The correct relationship between ${\mathrm{K}}_{{\mathrm{a}}_{1}},$ ${\mathrm{K}}_{{\mathrm{a}}_{2}}$ $\mathrm{and}$ ${\mathrm{K}}_{{\mathrm{a}}_{3}}$ is:

1. ${\mathrm{K}}_{{\mathrm{a}}_{3}}={\mathrm{K}}_{{\mathrm{a}}_{1}}×{\mathrm{K}}_{{\mathrm{a}}_{2}}$

2. ${\mathrm{K}}_{{\mathrm{a}}_{3}}={\mathrm{K}}_{{\mathrm{a}}_{1}}+{\mathrm{K}}_{{\mathrm{a}}_{2}}$

3. ${\mathrm{K}}_{{\mathrm{a}}_{3}}={\mathrm{K}}_{{\mathrm{a}}_{1}}-{\mathrm{K}}_{{\mathrm{a}}_{2}}$

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  Subtopic:  Introduction To Equilibrium |
72%
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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 , $\mathrm{Q}$ $=$ $\frac{{\left[{\mathrm{NH}}_{3}\right]}^{2}}{\left[{\mathrm{N}}_{2}\right]{\left[{\mathrm{H}}_{2}\right]}^{2}}$ .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 given 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  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 |
66%
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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 |
59%
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