Statement I: | Thermodynamic properties are macroscopic in nature. |
Statement II: | When a gas expands into a vacuum, the work done by it is zero. |
1. | Statement I is incorrect and Statement II is correct. |
2. | Both Statement I and Statement II are correct. |
3. | Both Statement I and Statement II are incorrect. |
4. | Statement I is correct and Statement II is incorrect. |
Assertion (A): | Heat energy is completely transformed into work during the isothermal expansion of a gas. |
Reason (R): | During an isothermal process, the changes in the internal energy of a gas due to a decrease in pressure are nullified by the changes due to an increase in volume. |
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. | Both (A) and (R) are False. |
Assertion (A): | \(C_p - C_v = R \), for 1 mole of an ideal gas. |
Reason (R): | R is equal to the work done when the temperature of one mole of an ideal gas is increased by 1º. |
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. | Both (A) and (R) are False. |
Assertion (A): | Work done in an irreversible isothermal process at constant volume is zero. |
Reason (R): | Work is assigned a negative sign during expansion and is assigned a positive sign during compression. |
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. | Both (A) and (R) are false. |
Statement I: | Total enthalpy change of a multistep process is the sum of ∆H1 + ∆H2 + ∆H3 + . . . |
Statement II: | When heat is absorbed by the system, the sign of q is taken to be negative. |
1. | Statement I is correct; Statement II is correct. |
2. | Statement I is correct; Statement II is incorrect. |
3. | Statement I is incorrect; Statement II is correct. |
4. | Statement I is incorrect; Statement II is incorrect. |
The correct statements among the following are :
a. | The enthalpy of two moles of ZnO is less than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ |
b. | The enthalpy of two moles of ZnO is more than the total enthalpy of two moles of Zn and one mole of oxygen by 693.8 kJ |
c. | 693 . 8 kJ mol -1 energy is evolved in the reaction |
d. | 693 . 8 kJ mol -1 energy is absorbed in the reaction |
1. (a, b)
2. (b, c)
3. (c, d)
4. (a, c)
A sample containing 1.0 mol of an ideal gas undergoes an isothermal, reversible expansion to ten times its original volume in two separate experiments. The expansion is carried out at temperatures of 300 K and 600 K, respectively.
The correct statements among the following are:
(a) | Work done at 600 K is 20 times the work done at 300 K. |
(b) | Work done at 300 K is twice the work done at 600 K. |
(c) | Work done at 600 K is twice the work done at 300 K. |
(d) | ∆ U = 0 in both cases. |
1. (a) and (b)
2. (b) and (c)
3. (c) and (d)
4. (a) and (d)
For the graph given below, it can be concluded that work done during the process shown will be-
1. | Zero | 2. | Negative |
3. | Positive | 4. | Cannot be determined |
Consider the following graph.
The work done, as per the graph above, is:
1. | Positive | 2. | Negative |
3. | Zero | 4. | Cannot be determined |
1.0 mol of a monoatomic ideal gas is expanded from state (1) to state (2) as shown in the graph below:
The work done for the expansion of gas from state (1) to state (2) at 298 K will be:
1. 1617.6 J
2. -1617.6 J
3. 1717.6 J
4. -1717.6 J