Q. No.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 |
(U: internal energy, S: entropy, p: pressure, V: volume, R: gas constant)
(Given : molar heat capacity at constant volume, \(C_{v,m}\) of the gas is \({ 5 \over 2 }R\))
1. 5
2. 10
3. 0.1
4. 0.5
What is a necessary condition for an adiabatic process to occur?
1. ∆T = 0
2. ∆P = 0
3. q = 0
4. w = 0
Which, among the following, is not a state function?
1. Internal energy
2. Free energy
3. Work
4. Enthalpy
Identify the false statement among the following.
| 1. | Temperature is a state function. |
| 2. | Work is a state function. |
| 3. | Change in the state is completely defined when the initial and final states are specified. |
| 4. | Work appears at the boundary of the system. |
The enthalpy of formation of all elements in their standard state is-
| 1. | Unity | 2. | Zero |
| 3. | Less than zero | 4. | Different for each element |
Thermodynamics is not concerned about which of the following?
| 1. | Energy changes involved in a chemical reaction. |
| 2. | The extent to which a chemical reaction proceeds. |
| 3. | The rate at which a reaction proceeds. |
| 4. | The feasibility of a chemical reaction. |
Calculate the correct values of heat transfer (q), change in temperature (ΔT), and work done (W) for the free expansion of an ideal gas under adiabatic conditions.
1. q = 0, ΔT ≠ 0, W = 0
2. q ≠ 0, ΔT = 0, W = 0
3. q = 0, ΔT = 0, W = 0
4. q = 0, ΔT = 0, W ≠ 0
Calculate the amount of heat required to raise the temperature of 60.0 g of aluminium from 35°C to 55°C.
(Molar heat capacity of Al = 24 J mol⁻¹ K⁻¹; molar mass of Al = 27 g mol⁻¹)
| 1. | \(1 . 07\) \(J\) | 2. | \(1 . 07\) \(kJ\) |
| 3. | \(106 . 7\) \(kJ\) | 4. | \(100 . 7\) \(kJ\) |
Which among the following statements about open, closed, and isolated systems is correct?
| 1. | The presence of reacting species in a covered beaker represents an open system. |
| 2. | In a closed system, there is an exchange of both energy and matter between the system and its surroundings. |
| 3. | A system containing reactants in a closed vessel made of copper is an example of a closed system. |
| 4. | A system containing reactants in a thermos flask or any other closed, insulated vessel is an example of a closed system. |
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