The work done during the expansion of a gas from a volume of 4 dm3 to 6 dm3 against a constant external pressure of 3 atm is:
1. –608 J
2. +304 J
3. –304 J
4. –6 J
for the following reaction is:
1. | -731 J | 2. | -1317 J |
3. | -501 J | 4. | +731 J |
At 27ºC latent heat of fusion of a compound is 2930 J/mol. Entropy change is:
1. 9.77 J/mol K
2. 10.77 J/mol K
3. 9.07 J/mol K
4. 0.977 J/mol K
For the reaction
C2H5OH(l) + 3O2(g) →2CO2(g) + 3H2O(l) which one is true:
1. | ∆H = ∆E – RT | 2. | ∆H = ∆E + RT |
3. | ∆H = ∆E + 2RT | 4. | ∆H = ∆E – 2RT |
Unit of entropy is:
1. JK–1 mol–1
2. J mol–1
3. J–1K–1 mol–1
4. JK mol–1
In a closed insulated container a liquid is stirred with a paddle to increase the temperature. The correct option regarding this among the following is:
1. ∆E = W ≠ 0, q = 0
2. ∆E = W = q ≠ 0
3. ∆E = 0, W = q ≠ 0
4. W = 0 , ∆E = q ≠ 0
Heat of combustion ∆Hº for C(s), H2(g) and CH4(g) are – 94, – 68 and – 213 Kcal/mol. ∆Hº for C(s) + 2H2(g) → CH4 (g) is:
1. | – 17 Kcal | 2. | – 111 Kcal |
3. | – 170 Kcal | 4. | – 85 Kcal |
For the given reaction
, the heat of formations of are -188 kJ/mol & -286 KJ/mol respectively. The change in the enthalpy of the reaction will be:
1. – 196 kJ/mol
2. + 196 kJ/mol
3. + 948 kJ/mol
4. – 948 kJ/mol
When 1 mol gas is heated at constant volume, the temperature is raised from 298 to 308 K. Heat supplied to the gas is 500 J. The correct statement among the following is:
1. q = w = 500 J, ∆U = 0
2. q = ∆U = 500 J, w = 0
3. q = w = 500 J, ∆U = 0
4. ∆U = 0, q = w = – 500 J
Enthalpy of is negative. If the enthalpy of combustion of are x and y respectively, then which relation is correct:
1. | x > y | 2. | x < y |
3. | x = y | 4. | x ≥ y |