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For the reaction,${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NH}}_3$ , the value of
equilibrium constant is K₁ then the
equilibrium constant for the reaction,
${\mathrm{NH}}_3\left(\mathrm{g}\right)\rightleftharpoons \frac{1}{2}{\mathrm{N}}_2\left(\mathrm{g}\right)+\frac{3}{2}{\mathrm{H}}_2\left(\mathrm{g}\right)$ will be
1. $\frac{1}{{\mathrm{K}}_1}$
2. $\frac{1}{2{\mathrm{K}}_1}$
3. $\frac{2}{{\mathrm{K}}_1}$
4. $\frac{1}{\sqrt{{\mathrm{K}}_1}}$

For the reaction,
${\mathrm{NH}}_2{\mathrm{COONH}}_4\left(\mathrm{s}\right)\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$, the
equilibrium pressure is 15 atmosphere. The
value of K_p is
1. 15 atm³
2. 50 atm³
3. 500 atm³
4. 100 atm³

For the reaction,
${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ on adding
inert gas at constant volume, equilibrium
1. Shifts in forward direction
2. Shifts in backward direction
3. Unaffected
4. Initially in forward direction

$\mathrm{A}\left(\mathrm{g}\right)+3\mathrm{B}\left(\mathrm{g}\right)\rightleftharpoons 4\mathrm{C}\left(\mathrm{g}\right)$ Initial
concentration of A is equal to that of B. The
equilibrium concentration of A and C are
equal. K_c is
1. 0.08
2. 0.8
3. 8
4. 80

The strongest conjugate base is
1. CH3COO^-
2. ${\mathrm{NO}}_3^{-}$
3. Cl^-
4. ${\mathrm{HSO}}_4^{-}$

The equilibrium constant (Kp) for the
reaction,$2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right)$
at 1000K is 3.5 atm^–1. What would be the
partial pressure of oxygen gas, if the
equilibrium is found to have equal moles
of SO₂ and SO₃?
1. 0.35 atm
2. 3.5 atm
3. 2.85 atm
4. 0.285 atm

In the dissociation of PCl₅ as
${\mathrm{PCl}}_5\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{PCl}}_3\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)$ if the degree
of the dissociation is $\mathrm{\alpha }$ at equilibrium
pressure P, then the equilibrium constant
for the reaction
1. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^2}{1+{\mathrm{\alpha }}^2\mathrm{P}}$
2. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^2{\mathrm{P}}^2}{1-{\mathrm{\alpha }}^2}$
3. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha P}}^2}{1-{\mathrm{\alpha }}^2}$
4. ${\mathrm{K}}_{\mathrm{p}}=\frac{{\mathrm{\alpha }}^2\mathrm{P}}{1-{\mathrm{\alpha }}^2}$

For the reaction
2A(g) + B(g)$\rightleftharpoons$3C(g) + D(g)
Two moles each of A and B were taken
into a 1L flask. The following must always
be true when the system attained
equilibrium
1. [A] = [B]
2. [A] < [B]
3. [B] = [C]
4. [A] + [B] < [C] + [D]

Which of the following reactions is
favoured by increased of temperature?
1. ${\mathrm{N}}_2+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3+22.9 \mathrm{kcl}$
2. ${\mathrm{N}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2\mathrm{NO}\left(\mathrm{g}\right)-42.8 \mathrm{kcl}$
3. $2{\mathrm{SO}}_2\left(\mathrm{g}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{SO}}_3\left(\mathrm{g}\right)+45.3 \mathrm{kcl}$
4. ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{Cl}}_2\left(\mathrm{g}\right)-44.0 \mathrm{kcl}\rightleftharpoons 2 \mathrm{HCl}\left(\mathrm{g}\right)$

Given a hypothetical reaction :
${\mathrm{AB}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{B}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{AB}}_3\left(\mathrm{g}\right);$ $∆\mathrm{H}=-\mathrm{x}$ $\mathrm{kJ}$
More AB₃​ could be produced at equilibrium by :

Inert gas has been added to the following
equilibrium system at constant volume
${\mathrm{SO}}_2\left(\mathrm{g}\right)+\frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right)$
To which direction will the equilibrium shift ?
1. Forward
2. Backward
3. No effect
4. Unpredictable

One mole of N₂ is mixed with 3 moles of
H₂ in one litre container. If 50% of N₂ is
converted into ammonia by the reaction
N₂ (g) + 3H₂ (g)$\rightleftharpoons$2NH₃ (g) , then the total
number of moles of gas at the equilibrium
are
1. 1.5
2. 4.5
3. 3.0
4. 6.0

In the following equilibria
I : A + 2B$\rightleftharpoons$C;K_eq = K₁
II : C+ D$\rightleftharpoons$3A;Keq = K₂
III : 6B + D$\rightleftharpoons$2C;Keq = K₃
Hence,
1. 3K₁ + K₂ = K₃
2. ${\mathrm{K}}_1^3.{\mathrm{K}}_2^2={\mathrm{K}}_3$
3. $3{\mathrm{K}}_1+{\mathrm{K}}_2^2={\mathrm{K}}_3$
4. ${\mathrm{K}}_1^3.{\mathrm{K}}_2={\mathrm{K}}_3$
 

For the following gaseous equilibria X, Y
and Z at 300K
$\mathrm{X}: 2{\mathrm{SO}}_2+{\mathrm{O}}_2\rightleftharpoons 2{\mathrm{SO}}_3$
$\mathrm{Y}:{\mathrm{PCl}}_5\rightleftharpoons {\mathrm{PCl}}_3+{\mathrm{Cl}}_2$
$\mathrm{Z}: 2\mathrm{HI}\rightleftharpoons {\mathrm{H}}_2+{\mathrm{I}}_2$
Ratio of K_p and K_c in the increasing order
is:
1. X = Y = Z
2. X < Y < Z
3. X < Z < Y
4. Z < Y < X

4 moles of A are mixed with 4 moles of B,
when 2 moles of C are formed at
equilibrium according to the reaction
$\mathrm{A}+\mathrm{B}\rightleftharpoons \mathrm{C}+\mathrm{D}$
The value of equilibrium constant is:
1. 4
2. 1
3. 1/2
4. 1/4