If the equilibrium constant for N2(g) + O2 (g) ⇄ 2NO(g) is K, the equilibrium constant for $$\frac{1}{2}$$N2(g) + $$\frac{1}{2}$$O2(g) ⇄ NO(g) will be?

1. ${K}^{\frac{1}{2}}$

2. $\frac{1}{2}K$

3. K

4. ${K}^{2}$

Subtopic:  Kp, Kc & Factors Affecting them |
84%
From NCERT
NEET - 2015
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The value of the equilibrium constant for a particular reaction is 1.6 × 1012. When the system is in equilibrium, it will include:
1. All reactants
2. Mostly reactants
3. Mostly products
4. Similar amounts of reactants and products

Subtopic:  Kp, Kc & Factors Affecting them |
71%
From NCERT
NEET - 2015
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For a given exothermic reaction, Kp and Kp are the equilibrium constants at temperatures T1 and Trespectively. Assuming that the heat of reaction is constant in temperatures range between T1 and T2, it is a readily observation that:
1. ${K}_{p}>{K}_{p}^{\text{'}}$
2. ${K}_{p}<{K}_{p}^{\text{'}}$
3. ${K}_{p}={K}_{p}^{\text{'}}$
4. ${K}_{p}=\frac{1}{{K}_{p}^{\text{'}}}$

Subtopic:  Kp, Kc & Factors Affecting them |
55%
AIPMT - 2014
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Given that the equilibrium constant for the reaction

$2S{O}_{2\left(g\right)}$ $+$ ${O}_{2\left(g\right)}$ $⇋$ $2S{O}_{3\left(g\right)}$ 

has a value of 278 at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be:

$S{O}_{3\left(g\right)}$  $⇋$ $S{O}_{2\left(g\right)}$ $+$ $1/2$ ${O}_{2\left(g\right)}$ 

1.  $3.6$ $×$ ${10}^{-3}$ 

2.  $6.0$ $×$ ${10}^{-2}$ 

3.  $1.3$ $×$ ${10}^{-5}$ 

4.  $1.8$ $×$ ${10}^{-3}$ 

Subtopic:  Kp, Kc & Factors Affecting them |
72%
From NCERT
AIPMT - 2012
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Consider the following reaction:
A2(g) + B2(g)  ⇋ 2AB(g)
At equilibrium, the concentrations of  A2 = 3.0×10–3 M;  B2 = 4.2×10–3 M and AB = 2.8×10–3M.
The value $$K_C$$ for the above-given reaction in a sealed container at 527°C is:

 1 3.9 2 0.6 3 4.5 4 2
Subtopic:  Kp, Kc & Factors Affecting them |
82%
From NCERT
AIPMT - 2012
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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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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%
From NCERT
AIPMT - 2010
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The reaction-

$2A+B\left(g\right)$ $⇌$ $3C\left(g\right)+D\left(g\right)$

begins with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:

1. $\left[{\left(0.75\right)}^{3}\left(0.25\right)\right]÷\left[{\left(0.50\right)}^{2}\left(0.75\right)\right]$

2. $\left[{\left(0.75\right)}^{3}\left(0.25\right)\right]÷\left[{\left(0.50\right)}^{2}\left(0.25\right)\right]$

3. $\left[{\left(0.75\right)}^{3}\left(0.25\right)\right]÷\left[{\left(0.75\right)}^{2}\left(0.25\right)\right]$

4. $\left[{\left(0.75\right)}^{3}\left(0.25\right)\right]÷\left[{\left(1.00\right)}^{2}\left(1.00\right)\right]$

Subtopic:  Kp, Kc & Factors Affecting them |
66%
From NCERT
AIPMT - 2010
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The dissociation constants for acetic acid and HCN at 25 °C are 1.5 x 10-5 and 4.5 x 10-10, respectively. The equilibrium constant for the equilibrium,
CN- + CH3COOH  ⇌  HCN + CH3COO-
would be:
1. $3.0×{10}^{5}$
2. $3.0×{10}^{-5}$
3. $3.0×{10}^{-4}$
4. $3.0×{10}^{4}$

Subtopic:  Kp, Kc & Factors Affecting them |
From NCERT
AIPMT - 2009
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The dissociation equilibrium of a gas AB2 can be represented as
$2A{B}_{2}\left(g\right)$ $⇋$ $2AB\left(g\right)$ $+$ ${B}_{2}\left(g\right)$ 
The degree of dissociation is ‘x’ and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant KP and total pressure p is:
1. (2KP/p)
2. (2Kp /p)1/3
3. (2KP/p)1/2
4. (KP/P)

Subtopic:  Kp, Kc & Factors Affecting them |
69%
From NCERT
AIPMT - 2008
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