Q. No.An ideal gas goes from \(A\) to \(B\) via two processes, \(\mathrm{I}\) and \(\mathrm{II},\) as shown. If \(\Delta U_1\) and \(\Delta U_2\) are the changes in internal energies in processes \(\mathrm{I}\) and \(\mathrm{II},\) respectively, (\(P:\) pressure, \(V:\) volume) then:
1.
\(∆U_1 > ∆U_2\)
2.
\(∆U_1 < ∆U_2\)
3.
\(∆U_1 = ∆U_2\)
4.
\(∆U_1 \leq ∆U_2\)
The pressure-temperature \((P\text-T)\) graph for two processes, \(A\) and \(B,\) in a system is shown in the figure. If \(W_1\) and \(W_2\) are work done by the gas in process \(A\) and \(B\) respectively, then:
| 1. | \(W_{1}=W_2\) | 2. | \(W_{1}<W_2\) |
| 3. | \(W_{1}>W_2\) | 4. | \(W_{1}= - W_2\) |
Which of the following reactions has the least difference between the change in enthalpy (∆H) and the change in internal energy (∆E) at a given temperature?
1. \(2 \mathrm{SO}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \rightarrow 2 \mathrm{SO}_3(\mathrm{~g})\)
2. \(\mathrm{CaCO}_3(s) \rightarrow \mathrm{CaO}(s)+\mathrm{CO}_2(g)\)
3. \(\mathrm{NH}_4 \mathrm{SH} (s) ~~\rightarrow ~\mathrm{NH}_3(g)+\mathrm{H}_2 \mathrm{~S}(g)\)
4. \(2 \mathrm{NH}_3 (g) ~\rightarrow ~\mathrm{N}_2(g)+3 \mathrm{H}_2(g)\)
A system that can neither exchange matter nor energy with the surroundings is classified as:
1. Open system
2. Isolated system
3. Closed system
4. Both (1) & (2)
1. \(5:3\)
2. \(5:2\)
3. \(1:1\)
4. \(5:7\)
1. \(V_1= V_2\)
2. \(V_1> V_2\)
3. \(V_1< V_2\)
4. \(V_1\ge V_2\)
\(0.04\) mole of an ideal monatomic gas is allowed to expand adiabatically so that its temperature changes from \(800~\text{K}\) to \(500~\text{K}.\) The work done during expansion is nearly equal to:
| 1. | \(129.6~\text J\) | 2. | \(-129.6~\text J\) |
| 3. | \(149.6~\text J\) | 4. | \(-149.6~\text J\) |
The standard enthalpies of the formation of NO2(g) and N2O4(g) are 8 kcal mol–1 and 2 kcal mol–1 respectively. The heat of dimerization of NO2 in the gaseous state is:
| 1. | 10 k cal mol–1 | 2. | 6.0 k cal mol–1 |
| 3. | –14 k cal mol–1 | 4. | –6.0 k cal mol–1 |
Calculate the Gibbs energy change when 1 mole of NaCl is dissolved in water at 298 K. Given,
a. Lattice energy of NaCl = 778 kJ mol-1
b. Hydration energy of NaCl =-774.3 kJ mol-1
c. Entropy change at 298 K = 43 JK-1 mol-1
| 1. | -3.7 kJ | 2. | -9.1 kJ |
| 3. | -43 kJ | 4. | -13.14 kJ |
© 2025 GoodEd Technologies Pvt. Ltd.