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

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

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]

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

Determine the degree of hydrolysis in the hydrolytic equilibrium:
${\mathrm{A}}^{-}+{\mathrm{H}}_2\mathrm{O}\rightleftharpoons \mathrm{HA}+{\mathrm{OH}}^{-}$ 
given that the salt concentration is 0.001 M .
 (Given K_a = 1 × 10^–5)

1. 1 × 10^–3

2. 1 × 10^–4

3. 5 × 10^–4

4. 1 × 10^–6

The pH of a 0.01 M solution of acetic acid having
degree of dissociation 12.5% is
1. 5.623

2. 2.903

3. 3.723

4. 4.509

Which may be added to one litre of water to act
as a buffer
1. One mole of HC₂H₃O₂ and 0.5 mole of NaOH
2. One mole of NH₄Cl and one mole of HCl
3. One mole of NH₄OH and one mole of NaOH
4. One mole of HC₂H₃O₂ and one mole of HCl

A solution of weak acid HA containing 0.01 moles
of acid per litre of solutions has pH = 4. The
percentage degree of ionisation of the acid and
the ionisation constant of acid are respectively

1. 1%, 10^–6

2. 0.01%, 10^–4

3. 1%, 10^–4

4. 0.01%, 10^–6