(∆H - ∆E) for the formation of carbon monoxide (CO) from its elements at 298 K is (R = 8.314 JK -1 mol -1)
-2477.57 J mol -1
2477.57 J mol -1
-1238.78 J mol -1
1238.78 J mol -1
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 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
When the heat of a reaction at constant pressure is -2.5 × 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
The Van’t Hoff reaction isotherm is
∆G = RT log Kp
–∆G = RT In Kp
∆G = RT2 In Kp
None of these
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
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
When one mole of monoatomic ideal gas at T K undergoes adiabatic change under a constant external pressure of 1 atm, changes volume from 1L to 2L. The final temperature in Kelvin would be
T
A gas occupies 2 liter at STP. It is provided 300 J heat so that its volume becomes 2.5 liter at 1 atm. What will be the change of its internal energy?
-50.65 J
149.65 J
300 J
249.35 J
The molar heat capacity of water at constant pressure is 75 JK -1 mol -1. When 1.0 kJ of heat is supplied to 100 g of water, which is free to expand, the increase in temperature of water is
1.2 K
2.4 K
4.8 K
6.8 K
