The Van’t Hoff reaction isotherm is
∆G = RT log Kp
–∆G = RT In Kp
∆G = RT2 In Kp
None of these
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
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
What will be the change of entropy ΔrS° at 298 K for the reaction in which urea is formed from NH3 and CO2?2NH3 (g) + CO2 (g) → NH2CONH2(aq) + H2O(l)[Given the standard entropy of NH2CONH2(aq), CO2 (g), NH3 (g) and H2O(l) are 174.0, 213.7, 192.3 and 69.9 J K-1 mol-1 respectively]
200 JK-1 mol-1
-35.44 JK-1 mol-1
-354.4 JK-1 mol-1
425.2 JK-1 mol-1
2 moles of an ideal gas at 27oC are expanded reversibly from 2 L to 20 L. Find entropy change. (R = 2 cal/ mol K)
0
4
9.2
92.0
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
For the process
H2O(I) ( 1 bar, 273 K) → H2O(g) (1 bar, 373 K)
The correct set of thermodynamic parameters is
∆G = 0,∆S = +ve
∆G = 0, ∆S = -ve
∆G = +ve, ∆S = 0
∆G = -ve, ∆S = +ve
When the system is returned from state B to A along the curved path, work done on the system is 20J. Does the system absorb or liberate heat, and how much?
System liberates heat, -70J
System absorbs heat, 70J
System absorbs heat, 90J
System liberates heat, -90J
A monoatomic ideal gas undergoes a process in which the ratio of p to V at any instant is constant and equals to 1. What is the molar heat capacity of the gas?
4R / 2
3R / 2
5R / 2s
Zero
