The correct statement for a reversible process in a state of equilibrium is:
1. G = – 2.30RT log K
2. G = 2.30RT log K
3. Go = – 2.30RT log K
4. Go = 2.30RT log K
From the following bond energies:
H—H bond energy: 431.37 kJ mol-1
C=C bond energy: 606.10 kJ mol-1
C—C bond energy: 336.49 kJ mol-1
C—H bond energy: 410.50 kJ mol-1
Enthalpy for the reaction,
will be:
1. | 1523.6 kJ mol-1 | 2. | -243.6 kJ mol-1 |
3. | -120.0 kJ mol-1 | 4. | 553.0 kJ mol-1 |
The values of ΔH and ΔS for the given reaction are 170 kJ and 170 JK-1, respectively.
C(graphite) + CO2(g)→2CO(g)
This reaction will be spontaneous at:
1. 710 K
2. 910 K
3. 1110 K
4. 510 K
1. 1.968 V
2. 2.0968 V
3. 1.0968 V
4. 0.0968 V
Which of the following is correct for isothermal expansion of an ideal gas:
1. Wrev = Wirr
2. Wrev + Wirr = 0
3. Wrev > Wirr
4. qrev = qirr
Which, among the following, is not a state function?
1. Internal energy
2. Free energy
3. Work
4. Enthalpy
Which among the following state functions is an extensive property of the system?
1. | Temperature | 2. | Volume |
3. | Refractive index | 4. | Viscosity |
The bond energies of , C-H, H-H, and C=C are 198, 98, 103 and145 kcal respectively.
The enthalpy change of the reaction would be-
1. 48 kcal
2. 96 kcal
3. -40 kcal
4. -152 kcal
For the reaction, , at 298K is 164 kJ mol-1. The of the reaction is-
1. \(166.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
2. \(141.5 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
3. \(104.0 \mathrm{~kJ} \mathrm{~mol}^{-1} \)
4. \(-169 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
As an isolated box, equally partitioned, contains two ideal gasses A and B as shown:
When the partition is removed, the gases mix. The changes in enthalpy and entropy in the process, respectively, are
1. Zero, positive
2. Zero, negative
3. Positive, zero
4. Negative, zero