Spontaneous adsorption of a gas on solid surface is an exothermic process because
∆H increases for system
∆S increases for gas
∆S decreases for gas
∆G increases for gas.
When 1.8 g of steam at the normal boiling point of water is converted into water, at the same temperature, enthalpy and entropy changes respectively will be.[Given Δ Hvap for water = 40.8 kJ mol -1]
-8.12 kJ, 11.89 JK-1
10.25 kJ, 12.95 JK-1
-4.08 kJ, -10.93 JK-1
10.93 kJ, -4.08 JK-1
In which process net work done is zero?
Cyclic
Isobaric
Adiabatic
Free expansion
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 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
Mercury thermometer can be used to measure temperature up to
260oC
100oC
360oC
500oC
The heat of sublimation of iodine is 24 cal g-1 at 50oC. If specific heat of solid iodine and its vapours are 0.055 and 0.031 cal g-1 respectively, the heat of sublimation of iodine at 100oC is
22.8 cal g-1
25.2 cal g-1
-22.8 cal g-1
-25.2 cal g-1
In which case, a spontaneous reaction is possible at any temperature?
∆H –ve, ∆S +ve
∆H –ve, ∆S –ve
∆H +ve, ∆S +ve
None of these.
The Van’t Hoff reaction isotherm is
∆G = RT log Kp
–∆G = RT In Kp
∆G = RT2 In Kp
None of these
For a spontaneous reaction the ∆G, equilibrium constant (K) and Eocell will be respectively
–ve, > 1, -ve
–ve, < 1, -ve
+ve, > 1, -ve
–ve, > 1, +ve
