One mole of H2O and one mole of CO are taken in a 10 L vessel and heated to 725 K. At equilibrium, 40% of water(by mass) reacts with CO according to the equation,
H2O (g) + CO (g) H2 (g) + CO2 (g)
The equilibrium constant for the above-mentioned reaction would be:
1. | 0.66 | 2. | 0.35 |
3. | 0.44 | 4. | 0.82 |
The equilibrium pressure of C2H6 when it is placed in a flask at 4.0 atm pressure at 899 K would be:
C2H6 (g) C2H4 (g) + H2 (g)
(Kp = 0.04 atm at 899 K)
1. | 4.12 atm | 2. | 3.62 atm |
3. | 1.54 atm | 4. | 2.16 atm |
A sample of pure PCl5 was introduced into an evacuated vessel at 473 K.
After equilibrium was attained, a concentration of PCl5
was found to be 0.5 × 10–1 mol L–1. If the value of
Kc is 8.3 × 10–3 mol L–1, the concentrations of
PCl3 and Cl2 at equilibrium would be:
PCl5 (g) PCl3 (g) + Cl2(g)
1. | |
2. | |
3. | |
4. |
\(\mathrm{K}_{\mathrm{c}}=\frac{\left[\mathrm{NH}_3\right]^4\left[\mathrm{O}_2\right]^5}{[\mathrm{NO}]^4\left[\mathrm{H}_2 \mathrm{O}]^6\right.}\)
The balanced chemical equation corresponding to the above-mentioned expression is:
1. | \(4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 4 \mathrm{NH}_{3(\mathrm{g})}+5 \mathrm{O}_{2(\mathrm{g})} \) |
2. | \(4 \mathrm{NH}_3(\mathrm{g})+5 \mathrm{O}_{2(\mathrm{g})} \rightleftharpoons 4 \mathrm{NO}_{(\mathrm{g})}+6 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})}\) |
3. | \(\ 2 \mathrm{NO}_{(\mathrm{g})}+3 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 4 \mathrm{NH}_{3(\mathrm{g})}+3 \mathrm{O}_{2(\mathrm{g})}\) |
4. | \(\ \mathrm{NH}_{3(\mathrm{g})}+3 \mathrm{H}_2 \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{NO}_{(\mathrm{g})}+3 \mathrm{O}_{2(\mathrm{g})}\) |
For the following equilibrium, Kc= 6.3 × 1014 at 1000 K
The value of Kc for the reverse reaction is:
For the reaction, 2NOCl (g) 2NO (g) + Cl2 (g); Kp= 1.8 × 10–2 atm at 500 K.
The value of Kc for above mentioned reaction would be:
At 450 K, Kp= 2.0 × 1010 bar-1 for the given reaction at equilibrium
The value of Kc at this temperature would be :
For the reaction: at 1050 K. If the initial partial pressures are pCO= 1.4 atm and = 0.80 atm, the partial pressure of CO2 at equilibrium at 1050 K would be:
1. | 4.61 atm | 2. | 1.74 atm |
3. | 0.46 atm | 4. | 0.17 atm |
For the reaction,
at 500K. At a particular instant of time, [N2] = 3.0 mol L–1, [H2] = 2.0 mol L–1 and
[NH3] = 0.5 mol L–1 .
True statement among the following is:
1. Reaction is at equilibrium.
2. Reaction will proceed in the forward direction.
3. Reaction will proceed in the backward direction.
4. Can't predict the direction of the reaction.
At 1127 K and 1 atm pressure, a gaseous mixture of CO and CO2 in equilibrium with solid carbon has 90.55% CO by mass.
At the specified temperature, Kc for this reaction would be: