The Van’t Hoff reaction isotherm is
∆G = RT log Kp
–∆G = RT In Kp
∆G = RT2 In Kp
None of these
One mole of a gas occupying 3 dm3 expands against constant external pressure of 1 atm to a volume of 13 dm3. The work done is
-10 atm dm3
-20 atm dm3
40 atm dm3
-50 atm dm3
The enthalpy of vaporization of liquid diethyl ether (C2H5)2O, is 26.0 kJ mol -1 at its boiling point (35oC). What will be the ∆S for conversion of liquid to vapour and vapour to liquid respectively?
+84.41 and -84.41 JK -1 mol -1
+80.90 and –68.83 JK -1 mol -1
-84.41 and +90.63 JK -1 mol -1
+68.83 and -84.41 JK -1 mol -1
When I mole of a gas is heated at constant volume, temperature is raised from 298 K to 308 k. Heat supplied to the gas is 500 J. Then, which statement is correct?
q = -W = 500J, ∆E = 0
q = W = 500J, ∆E = 0
q = ∆E = 500J, W = 0
∆E = 0, q = W = -500J
For a reaction
∆H = 30 kJ mol -1 and ∆S = 0.07 kJ K -1 mol -1 at 1 atm. The temperature up to which the reaction would not be spontaneous is
T < 400.08 K
T < 273.15 K
T < 428.57 K
T < 473.50 K
An ideal gas expands in volume from 10-3 m3 to 10-2 m3 at 300 K against a constant pressure of 105 Nm-2.
The work done is
800 kJ
900 kJ
270 kJ
-900 J
Latent heat of vaporization of a liquid at 500 K and 1 atm pressure is 10.0 kcal/mol. What will be the change in to internal energy (∆E) of 3 mole of liquid at same temperature ?
30 kcal
-54 kcal
27.0 kcal
50 kcal
The difference between heats of reaction at constant pressure and constant volume for the reaction; 2 C6H6(I) +15O2 (g) → 12CO2(g) + 6H2O(I) at 25oC in kJ is
-7.43
6.42
-6.42
12.80
When the heat of a reaction at constant pressure is -2.5 x 103 cals and entropy change for the reaction is
7.4 cal deg -1, it is predicted that the reaction at 25oC is
Reversible
Spontaneous
Non-spontaneous
Irreversible
Internal energy and pressure of a gas of unit volume are related as