$\mathrm{If A}$ $+$ $B$ $⇋$ $C$ $+$ $D$ $Cons\mathrm{tan}t$ $=$ ${K}_{1}$
$E$ $+$ $F$ $⇌$ $G$ $+$ $H$ $Cons\mathrm{tan}t$ $=$ ${K}_{2}$

then C + D + E + F ⇒ product. The constant of reaction will be:

1.  $\frac{{K}_{1}}{{K}_{2}}$

2.  $\frac{{K}_{2}}{K1}$

3. ${K}_{1}{K}_{2}$

4. None of these

Subtopic:  Kp, Kc & Factors Affecting them |
77%
From NCERT
AIPMT - 1998
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The equilibrium constant Kp for the following reaction is:

${{\mathrm{MgCO}}_{3}}_{\left(\mathrm{s}\right)}⇌{\mathrm{MgO}}_{\left(\mathrm{s}\right)}+{{\mathrm{CO}}_{2}}_{\left(\mathrm{g}\right)}$

1.

2. $\mathrm{Kp}={\mathrm{P}}_{{\mathrm{CO}}_{2}}×\frac{{\mathrm{P}}_{{\mathrm{CO}}_{2}}×{\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_{3}}}$

3. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{CO}}_{2}}+{\mathrm{P}}_{\mathrm{MgO}}}{{\mathrm{P}}_{{\mathrm{MgCO}}_{3}}}$

4. $\mathrm{Kp}=\frac{{\mathrm{P}}_{{\mathrm{MgCO}}_{3}}}{{\mathrm{P}}_{{\mathrm{CO}}_{2}}×{\mathrm{P}}_{\mathrm{MgO}}}$

Subtopic:  Kp, Kc & Factors Affecting them |
89%
From NCERT
AIPMT - 2000
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The correct relation between dissociation constants of a di-basic acid is:

1. $K{a}_{1}=K{a}_{2}$

2. $K{a}_{1}>K{a}_{2}$

3. $K{a}_{1}

4. $K{a}_{1}=\frac{1}{K{a}_{2}}$

Subtopic:  Kp, Kc & Factors Affecting them |
69%
From NCERT
AIPMT - 2000
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For any reversible reaction, if we increase the concentration of the reactants, the effect on equilibrium constant will:
1. Depend on the amount of concentration
2. Remain unchanged
3. Decrease
4. Increase

Subtopic:  Kp, Kc & Factors Affecting them |
81%
From NCERT
AIPMT - 2000
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The ionization constant of ${\mathrm{CH}}_{3}\mathrm{COOH}$ is 1.7 × ${10}^{-5}$ and the concentration of ions is 3.4 × ${10}^{-4}$. The initial concentration of ${\mathrm{CH}}_{3}\mathrm{COOH}$ will be:
1.  3.4 × ${10}^{-4}$
2.  3.4× ${10}^{-3}$
3.  6.8 × ${10}^{-4}$
4.  6.8 × ${10}^{-3}$

Subtopic:  Kp, Kc & Factors Affecting them |
63%
From NCERT
AIPMT - 2001
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For a reaction , ${\mathrm{BaO}}_{2}\left(\mathrm{s}\right)⇌\mathrm{BaO}\left(\mathrm{s}\right)+{\mathrm{O}}_{2}\left(\mathrm{g}\right)$; ∆H = + ve. At equilibrium condition, the pressure of O2 depends on the:

1. Increased mass of BaO2

2. Increased mass of BaO

3. Increased temperature on equilibrium.

4. Increased mass of BaO2 and BaO both.

Subtopic:  Kp, Kc & Factors Affecting them |
82%
From NCERT
AIPMT - 2002
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The reaction quotient (Q) 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:
1. Q = KC
2. Q < KC
3. Q > KC
4. Q = 0

(where KC is the equilibrium constant)

Subtopic:  Kp, Kc & Factors Affecting them |
74%
From NCERT
AIPMT - 2003
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