Equilibrium Tes...

Two systems, $$P{ Cl }_{ 5 }(g)\rightleftharpoons P{ Cl }_{ 3 }(g)+{ Cl }_{ 2 }(g)$$ and $$CO{ Cl }_{ 2 }(g)\rightleftharpoons CO(g)+{ Cl }_{ 2 }(g)$$ are simultaneously in equilibrium in a vessel at constant volume. If some $$CO(g)$$ is introduced in the vessel at constant volume, then at new equilibrium, the concentration of:

For the reaction, $${ H }_{ 2 }(g)+{ I }_{ 2 }(g)\rightleftharpoons 2HI(g)$$, the equilibrium constant $${K}_{p}$$ changes with:

In which of the following reactions, the increase in volume of the container will favour the formation of products?

Given the equilibrium system, $${ NH }_{ 4 }Cl(s)\rightleftharpoons { NH }_{ 4 }^{ + }(aq.)+{ Cl }^{ - }(aq.);\left( \Delta { H }^{ o }=+3.5kcal/mol \right) $$.
What change will shift the equilibrium to the right?

Consider this equilibrium, for which $$\Delta H< 0$$.
$$HgO(s)+4{ I }^{ - }(aq.)+{ H }_{ 2 }O(l)\rightleftharpoons {Hg{ I }_{ 4 }}^{ 2- }+2{ OH }^{ - }$$
Which changes will increase the equilibrium concentration $${Hg{ I }_{ 4} }^{ 2- }$$?
$$I$$. Increasing the mass of $$HgO(s)$$ present
$$II$$. Increasing $$\left[ { I }^{ - } \right] $$
$$III$$. Adding $$1\ M$$ $$HCl$$

An increase in temperature increases which of the following?
1. The rate constant of a reaction
2. The ionic product of water
3. The equilibrium constant of an exothermic reaction
Select the correct answer using the code given below.

Water gas, an individual fuel, consisting $$CO$$ and $${H}_{2}$$ in equimolar amounts is obtained by passing steam over red-hot carbon in accordance with the reaction:
$$C(s)+{ H }_{ 2 }O(g)\rightleftharpoons CO(g)+{ H }_{ 2 }(g);\Delta { H }=+130.5kJ\quad $$
The yield of water gas can be increased by:
(1) Reducing the total pressure of the system
(2) Increasing pressure of steam
(3) Raising the temperature
(4) Introducing hot carbon

The reaction, $$2S{ O }_{ 2 }(g)+{ O }_{ 2 }(g)\rightleftharpoons 2{ SO }_{ 3 }(g)$$ (Exothermic), will shift in forward direction by:

The addition of $$HCl$$ will not suppress the ionisation of:

A monoprotic acid in $$1.00M$$ solution is $$0.001$$% ionised. The dissociation constant of acid is: