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

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,
${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ 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

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