The thermodynamic stability of NO(g) based on the above data is:
1. Less than NO2(g)
2. More than NO2(g)
3. Equal to NO2(g)
4. Insufficient data
The entropy change in the surroundings when 1.00 mol of H2O(l) is formed under standard conditions is-
∆fHθ = –286 kJ mol–1
1. 952.5 J mol-1
2.
3.
4.
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 shown by the above-mentioned graph is-
1. | Positive | 2. | Negative |
3. | Zero | 4. | Cannot be determined |
Consider the following diagram for a reaction .
The nature of the reaction is-
1. Exothermic
2. Endothermic
3. Reaction at equilibrium
4. None of the above
Consider the following diagram for a reaction
The nature of the reaction is-
1. | Exothermic | 2. | Endothermic |
3. | Reaction at equilibrium | 4. | None of the above |
Which of the following options correctly represents the relationship between \(C_p \text { and } C_V\) for one mole of an ideal gas?
1. \(C_P=R C_V \)
2. \(C_V=RC_P \)
3. \(C_P+C_V=R \)
4. \(C_{\mathrm{P}}-\mathrm{C}_{\mathrm{V}}=\mathrm{R}\)
For irreversible expansion of an ideal gas under isothermal condition, the correct option is :
1.
2.
3.
4.
Two litres of 1 mol an ideal gas at a pressure of 10 atm expands isothermally at 25 °C into a vacuum until its total volume is 10 litres. The amount of heat absorbed during expansion is:
(Given: log 5 = 0.699)
1. 51. 39 atm L
2. 39.36 atm L
3. 37. 34 atm ml
4. 26. 49 atm L
Assuming the water vapour to be a perfect gas. When 1 mol of water at 100°C and 1 bar pressure is converted to ice at 0°C, the change in internal energy is-
(The enthalpy of fusion of ice = 6.00 kJ mol-1 , heat capacity of water = 4.2 J/g°C)
1. 13.56 kJ mol-1
2. -12.16 kJ mol-1
3. -13.56 kJ mol-1
4. 12.16 kJ mol-1