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

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

An acidic buffer cannot be formed by which of the following combinations is:

1. ${\mathrm{HClO}}_4$ $\mathrm{and}$ ${\mathrm{NaClO}}_4$
2. ${\mathrm{CH}}_3\mathrm{COOH}$ $\mathrm{and}$ ${\mathrm{CH}}_3\mathrm{COONa}$
3. ${\mathrm{H}}_2{\mathrm{CO}}_3$ $\mathrm{and}$ ${\mathrm{Na}}_2{\mathrm{CO}}_3$
4. ${\mathrm{H}}_3{\mathrm{PO}}_4$ $\mathrm{and}$ ${\mathrm{Na}}_3{\mathrm{PO}}_4$

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