The equilibrium of three reactions with their respective equilibrium constants are given below,
\( \begin{array}{lc} \mathrm{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3 & \mathrm{~K}_1 \\ \mathrm{~N}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO} & \mathrm{K}_2 \\ \mathrm{H}_2+\frac{1}{2} \mathrm{O}_2 \rightleftharpoons \mathrm{H}_2 \mathrm{O} & \mathrm{K}_3 \end{array} \)
The equilibrium constant (K) of the following reaction will be :
1. \( \frac{K_{2}K_{3}^{3}}{K_{1}}\)
2. \( \frac{K_{2}K_{3}}{K_{1}}\)
3. \( \frac{K_{2}^{3}K_{3}}{K_{1}}\)
4. \( \frac{K_{3}^{3}K_{1}}{K_{2}}\)
A 20-litre container at 400 K contains CO2 (g) at pressure 0.4 atm and an excess of SrO (neglecting the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container.
The maximum volume of the container, when the pressure of CO2 attains its maximum value will be:
(Given that: SrCO3(s) ⇋ SrO(s) + CO2(g) , Kp = 1.6 atm)
1. | 10 litre | 2. | 2 litre |
3. | 4 litre | 4. | 5 litre |
If the equilibrium constant for N2(g) + O2 (g) ⇄ 2NO(g) is K, the equilibrium constant for \(\frac{1}{2}\)N2(g) + \(\frac{1}{2}\)O2(g) ⇄ NO(g) will be?
1.
2.
3. K
4.
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
Given that the equilibrium constant for the reaction
has a value of 278 at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be:
1.
2.
3.
4.
Given reaction: A2(g) + B2(g) ⇋ 2AB(g)
At equilibrium, the concentrations of A2 = 3.0×10–3 M; B2 = 4.2×10–3 M and AB = 2.8×10–3M. If the reaction takes place in a sealed vessel at 527 °C, then the value of KC will be:
1. | 3.9 | 2. | 0.6 |
3. | 4.5 | 4. | 2.0 |
For the reaction the equilibrium constant is K1. The equilibrium constant is K2 for the reaction
The value of K for the reaction given below will be:
1.
2.
3.
4.