Equilibrium

According to Le Chatelier's principle, increasing pressure in a gaseous equilibrium favours:

1. Side with more gas molecules
2. Side with fewer gas molecules
3. No change
4. Liquid formation only

Buffer solutions resist changes in:

1. Pressure
2. Temperature
3. pH
4. Volume

The value of ionic product of water (Kw) at 25 degrees C is:

1. 10^-7
2. 10^-14
3. 10^-1
4. 1

The common ion effect is the suppression of:

1. Ionisation of weak electrolyte
2. Temperature change
3. Pressure change
4. Catalyst activity

A strong acid completely ionises in water. Which is a strong acid?

1. CH3COOH
2. HCl
3. NH4OH
4. H2CO3

The conjugate base of H2O is:

1. H3O+
2. OH-
3. H+
4. O2-

The value of Kc greater than 1 indicates:

1. Reactants are favoured
2. Products are favoured
3. Reaction stops
4. No equilibrium exists

A catalyst in an equilibrium reaction:

1. Changes equilibrium constant
2. Shifts equilibrium position
3. Speeds up both forward and reverse reactions
4. Stops reverse reaction

The equilibrium constant expression for H2 + I2 2HI is:

1. [HI]/[H2][I2]
2. [HI]^2/[H2][I2]
3. [H2][I2]/[HI]^2
4. [HI]^2/[H2]

The pH of a neutral solution at 25 degrees C is:

1. 0
2. 5
3. 7
4. 14

A reaction in which reactants and products are present together at equilibrium is:

1. Irreversible reaction
2. Reversible reaction
3. Decomposition reaction
4. Neutralisation reaction

The value of equilibrium constant depends on:

1. Concentration
2. Temperature
3. Pressure only
4. Volume only

According to Le Chatelier's principle, increasing the concentration of reactants shifts equilibrium:

1. Towards reactants
2. Towards products
3. Does not affect equilibrium
4. Stops reaction

The equilibrium constant for a reaction is represented by:

1. K
2. Kc
3. Keq
4. All of these

Chemical equilibrium is established when:

1. Reactants are completely converted into products
2. Forward and backward reaction rates become equal
3. Reaction stops completely
4. Concentration of reactants becomes zero