Vant Hoff's Equation and Effect of Temperature on Equilibrium Constant

Q. Consider the reaction : $2S{O}_2\left(g\right)+O_2\left(g\right)\rightleftharpoons 2S{O}_3\left(g\right);△H^o=-198kJ$
The favourable conditions for the forward reaction are:

1. Increasing temperature as well as pressure
2. Lowering the temperature and increasing the pressure
3. Lowering of temperature as well as pressure
4. Lowering the pressure and increasing the temperature

Q.

For the reaction $2NO\left(g\right)\rightleftharpoons N_2\left(g\right)+O_2\left(g\right),\Delta H=-180kJmo{l}^{-1}$. Which of the following facts does not hold well?

1. The volume changes at constant temperature do not affect the equilibrium constant

2. The dissociation of NO is favored less at high temperature

3. The pressure changes at constant temperature do not affect the equilibrium constant

4. The dissociation of NO is favored more at high temperature

Q. Which of the following is incorrect about the following reaction –
$2S{O}_2\left(g\right)+O_2\left(g\right)\leftrightharpoons 2S{O}_3\left(g\right)△H=-45kCal$

1. High pressure will be favorable for production of
2. High temperature will favor forward reaction.
3. Decreasing concentration will reduce the rate of backward reaction.
4. Doubling the volume of container while keeping temperature same, will shift the equilibrium in reverse direction.

Q.

The oxidation of $S{O}_2$ by $O_2$ to $S{O}_3$ is an exothermic reaction. The yield of $S{O}_3$ will be maximum if

1. Temperature is increased and pressure is kept constant

2. Temperature is reduced and pressure is increased

3. Both temperature and pressure are increased

4. Both temperature and pressure are reduced

Q. The reaction, $S{O}_2\left(g\right)+C{l}_2\left(g\right)\leftrightharpoons S{O}_{2}C{l}_2\left(l\right)$ is exothermic. A mixture of $S{O}_2,C{l}_2$ and $S{O}_{2}C{l}_2$ is at equilibrium in a closed container. Now, a certain amount of $S{O}_2$is added to the mixture, the volume remaining the same. Which of the following statement is true?

1. The pressure inside the container will not change
2. The temperature will not change
3. the temperature will decrease
4. The temperature will increase

Q.

In the reaction $N_2\left(g\right)+3H_2\left(g\right)\rightleftharpoons 2N{H}_3\left(g\right)$, the value of the equilibrium

constant depends on

1. The temperature

2. Volume of the reaction vessel

3. Total pressure of the system

4. The initial concentration of nitrogen and hydrogen

Q.

For an equilibrium reaction A (g) + B (g) $\rightleftharpoons$ C (g) + D (g), $\Delta H$ = -ve. An increase in temperature would cause

1. No change in the value of

2. A decrease in the value of

3. A change in which cannot be qualitatively predicted

4. An increase in the value of

Q.

\(N_2 ~+ ~O_2 ~\rightleftharpoons~ 2NO ~+~ (-Q cals)\)

In the above reaction which is the essential condition for the higher production of $NO$

1. High temperature

2. High pressure

3. Low temperature

4. Low pressure

Q. For the reaction H${}_2$ (g) + I${}_2$(g)$\rightleftharpoons$2HI(g), K${}^o$${}_c$= 66.9 at 350${}^{\circ }$C and K${}^o$${}_c$= 50.0 at 448 ${}^{\circ }$C. The reaction has

1. H = +ve.

2. H = -ve.

3. H whose sign cannot be predicted

4. H = Zero

Q.

For an equilibrium reaction A (g) + B (g)$\rightleftharpoons$ C (g) + D (g), $\Delta H$ = +ve. An increase in temperature would cause

1. An increase in the value of

2. No change in the value of

3. A change in which cannot be qualitatively predicted

4. A decrease in the value of