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

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 |
80%
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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 |
81%
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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 |
74%
From NCERT
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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 |
67%
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For the following reaction,
H2(g)+I2(g)2HI(g) $at$ $250°C,$

The effect on the state of equilibrium on doubling the volume of the system will be:

 1 Shift to the reactant side 2 Shift to the product side 3 No effect on the state of equilibrium 4 Liquefaction of HI

Subtopic:  Le Chatelier's principle |
83%
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Given a hypothetical reaction :
${\mathrm{AB}}_{2}\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{B}}_{2}\left(\mathrm{g}\right)⇌{\mathrm{AB}}_{3}\left(\mathrm{g}\right);$ $∆\mathrm{H}=-\mathrm{x}$ $\mathrm{kJ}$
More  could be produced at equilibrium by :

 1 Using a catalyst 2 Removing some of B2 gas 3 Increasing the temperature 4 Increasing the pressure
Subtopic:  Le Chatelier's principle |
75%
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(a) PCl5 (g) $⇋$ PCl3 (g) + Cl2 (g)

(b) CaO (s) + CO2 (g) $⇋$  CaCO3 (s)

(c) 3Fe (s) + 4H2O (g) $⇋$ Fe3O4 (s) + 4H2 (g)

The effect of an increase in the volume on the number of moles of products in the above-mentioned reactions would be, respectively:

1. a) Increase,  b) decrease, c) same

2. a) Decrease,  b) same, c) increase

3. a) Increase,  b) increase, c) same

4. a) Increase,  b) decrease, c) increase

Subtopic:  Le Chatelier's principle |
71%
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The equilibrium reaction that doesn't have equal values for Kc and Kis:

1. $$2NO(g) \rightleftharpoons N_2(g) + O_2(g)$$
2. $$SO_2(g) + NO_2(g) \rightleftharpoons SO_3(g) + NO(g)$$
3. $$H_2(g) + I_2(g) \rightleftharpoons 2HI (g)$$
4. $$2C(s) + O_2(g) \rightleftharpoons 2CO_2(g)$$

Subtopic:  Kp, Kc & Factors Affecting them |
91%
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AIPMT - 2010
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For the reaction ${\mathrm{N}}_{2}\left(\mathrm{g}\right)$ $+$ ${\mathrm{O}}_{2}\left(\mathrm{g}\right)⇋2\mathrm{NO}\left(\mathrm{g}\right)$ the equilibrium constant is K1. The equilibrium constant is K2 for the reaction  $2\mathrm{NO}\left(\mathrm{g}\right)$ $+$ ${\mathrm{O}}_{2}\left(\mathrm{g}\right)$ $⇋2{\mathrm{NO}}_{2}\left(\mathrm{g}\right)$ 
The value of K for the reaction given below will be:
${\mathrm{NO}}_{2}\left(\mathrm{g}\right)⇋\frac{1}{2}{\mathrm{N}}_{2}\left(\mathrm{g}\right)$ $+{\mathrm{O}}_{2}\left(\mathrm{g}\right)$ 

1.  $\frac{1}{4}$ $\left(4\right)$ ${\mathrm{K}}_{1}$ ${\mathrm{K}}_{2}$

2.  ${\left[\frac{1}{{\mathrm{K}}_{1}{\mathrm{K}}_{2}}\right]}^{1/2}$

3.  $\frac{1}{\left({\mathrm{K}}_{1}{\mathrm{K}}_{2}\right)}$

4.  $\frac{1}{\left(2{\mathrm{K}}_{1}{\mathrm{K}}_{2}\right)}$

Subtopic:  Kp, Kc & Factors Affecting them |
88%
From NCERT
AIPMT - 2011
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For the reaction 2NOCl(g)⇔2NO(g)+Cl2(g), KC at 427$°$C is $$3\times 10^{-6} \ mol\ L^{-1}$$. The value of Kp will be :

1. $1.72×{10}^{-4}$

2. $7.50×{10}^{5}$

3. $2.50×{10}^{-5}$

4. $2.50×{10}^{-4}$

Subtopic:  Kp, Kc & Factors Affecting them |
83%
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