Acidity of BF3 can be explained on the basis of:
1. Arrhenius concept
2. Bronsted Lowry concept
3. Lewis concept
4. Bronsted Lowry as well as Lewis concept
The mixture that will produce a buffer solution when mixed in equal volumes is:
1. | 0.1 mol dm-3 NH4OH and 0.1 mol dm-3 HCl |
2. | 0.05 mol dm-3 NH4OH and 0.1 mol dm-3 HCl |
3. | 0.1 mol dm-3 NH4OH and 0.05 mol dm-3 HCl |
4. | 0.1 mol dm-3 CH3COONa and 0.1 mol dm-3 NaOH |
1. solution
2. solution
3.
4. Aqueous ammonia
The value of the pH of \(0.01 \) \(\text{mol dm}^{-3} \)\(\text{CH}_3\text{COOH}\) \(\left(K_a=1.74 \times 10^{-5}\right)\) is:
1. | 3.4 | 2. | 3.6 |
3. | 3.9 | 4. | 3.0 |
Which of the following alternatives best describes the reaction A ⇌ B at its halfway point?
1. \(\Delta G^{\ominus}=0\)
2. \(\Delta G^{\ominus}>0\)
3. \(\Delta G^{\ominus}<0\)
4. \(\Delta G^{\ominus}=-RTlnK\)
On increasing the pressure, the direction in which the gas phase reaction proceeds to re-establish equilibrium is predicted by applying Le-Chatelier's principle. Consider the reaction,
Which of the following is correct, if the total pressure at which the equilibrium is established is increased without changing the temperature?
1. | K will remain the same. |
2. | K will decrease. |
3. | K will increase. |
4. | K will increase initially and then decrease, when pressure is very high. |
1. | H2(g)+I2(g)⇌2HI(g) |
2. | PCl5(g)⇌ PCl3(g)+Cl2(g) |
3. | N2(g)+3H2(g)⇌2NH3(g) |
4. | The equilibrium will remain unaffected in all the three cases. |
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.