1. | Possible at high temperature. |
2. | Possible only at low temperatures. |
3. | Not possible at any temperature. |
4. | Possible at any temperature. |
The work done when 1 mole of gas expands reversibly and isothermally from a pressure of 5 atm to 1 atm at 300 K is:
(Given log 5 = 0.6989 and R = 8.314 J K-1 mol-1)
1. zero J
2. 150 J
3. +4014.6 J
4. -4014.6 J
Assertion (A): | All combustion reactions are exothermic. |
Reason (R): | \({(\Sigma v_p\Delta_fH(P)> \Sigma v_R\Delta_fH(R))}\). | For an exothermic reaction, enthalpies of products are greater than enthalpies of reactants
1. | Both (A) and (R) are true and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are true but (R) is not the correct explanation of (A). |
3. | (A) is true but (R) is false. |
4. | (A) is false but (R) is true. |
Assertion (A): | The increase in internal energy \((\Delta E ) \) for the vapourisation of one mole of water at 1 atm and 373 K is zero. |
Reason (R): | For all isothermal processes, \(\Delta E = 0 \). |
1. | Both (A) and (R) are True and (R) is the correct explanation of (A). |
2. | Both (A) and (R) are True but (R) is not the correct explanation of (A). |
3. | (A) is True and (R) is False. |
4. | (A) and (R) both are False. |
List I | List II |
A. \(\Delta H = q \) | I. \(P_{ext} =0 \) |
B. Free expansion | II. Heat |
C. Path function | III. At constant pressure |
D. Reversible process | IV. An infinitely slow process that proceeds through a series of equilibrium states |
1. | Molar Heat | 2. | Specific Heat |
3. | Entropy | 4. | Heat capacity |
1. | 1.2 kJ | 2. | 0.16 kJ |
3. | 3.2 kJ | 4. | 1.6 kJ |