Temperature and Chemical Equilibrium

Q.

Consider the following reaction:

${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right);∆\mathrm{H}°=+58\mathrm{kJ}$

For each of the following cases (a, b), the direction in which the equilibrium shifts is:

(a) Temperature is decreased.

(b) Pressure is increased by adding ${\mathrm{N}}_2$ at constant $T$.

1. (a) towards reactant, (b) towards product

2. (a) towards reactant, (b) no change

3. (a) towards product, (b) towards reactant

4. (a) towards product, (b) no change

Q.

An exothermic reaction is favoured when the temperature is increased for a system in equilibrium.

1. True

2. False

Q.

Consider the following reaction:

$2S{O}_2\left(g\right)+O_2\left(g\right)\leftrightharpoons 2S{O}_3\left(g\right)+heat$

What will happen if the temperature of the reacting system is decreased?

1. More amount of sulphur trioxide will be formed.
2. Equilibrium will shift to the back.
3. No change
4. Less amount of sulphur dioxide will be formed.

Q.

At equilibrium, rate of the forward reaction is equal to the rate of the backward reaction

1. 1/3 times

2. 2/3 times

Q.

Consider the following reaction:

$2S{O}_2\left(g\right)+O_2\left(g\right)\leftrightharpoons 2S{O}_3\left(g\right)+heat$

If we increase the temperature of the given equilibrium system then an exothermic reaction will be favoured.

1. True

2. False

Q.

${\mathrm{KClO}}_3\underset{∆}{\overset{{\mathrm{MnO}}_2}{\to }}\mathrm{KCl}+{\mathrm{O}}_2$

For the above shown decomposition reaction of potassium chlorate, identify the incorrect statement:

1. The physical state of ${\mathrm{KClO}}_3$ is solid.

2. The physical state of ${\mathrm{O}}_2$ is gas.

3. The above reaction is balanced.

4. ${\mathrm{MnO}}_2$ plays the role of a catalyst.

Q. What is the Le chatelier's principle?

Q.

Consider the following reaction:

$N_2\left(g\right)+3H_2\left(g\right)\leftrightharpoons 2N{H}_3\left(g\right)$

What will happen if the temperature of the reacting system is decreased?

1. An exothermic reaction will be favored.

2. An endothermic reaction will be favored.

3. A forward reaction will be favored.

4. A backward reaction will be favored.

Q.

State and explain Le Chateliers principle. Apply the principle to the following equilibria.

(ii) $2{\mathrm{NH}}_3\rightleftharpoons {\mathrm{N}}_2+3{\mathrm{H}}_2-\text{Heat}$

Q.

Can reactions be forced to run backwards?

Q.

define Le Chateliers principle.

Q. Statement I: When the temperature of a reaction at equilibrium is increased, the equilibrium will shift to favor the endothermic direction
Because
Statement II: Endothermic reactions involve heat acting as a reactant and Le Chateliers principle states that an equilibrium shift will occur to offset temperature changes

1. T, T
2. T, F
3. F, T
4. F, F
5. Given information is insufficient.

Q.

Consider the following reaction:

$N_2\left(g\right)+3H_2\left(g\right)\leftrightharpoons 2N{H}_3\left(g\right)$

What will happen if the temperature of the reacting system is decreased?

1. An exothermic reaction will be favored.

2. An endothermic reaction will be favored.

3. A forward reaction will be favored.

4. A backward reaction will be favored.

Q.

An exothermic reaction is favoured when the temperature is increased for a system in equilibrium.

1. True

2. False

Q.

Consider the following reaction:

$2S{O}_2\left(g\right)+O_2\left(g\right)\leftrightharpoons 2S{O}_3\left(g\right)+heat$

If we increase the temperature of the given equilibrium system then an exothermic reaction will be favoured.

1. False

2. True