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 |
An enthalpy diagram for a particular reaction is given below:
The correct statement among the following is-
1. Reaction is spontaneous
2. Reaction is non-spontaneous
3. Cannot predict spontaneity of the reaction from the graph given above
4. None of the above
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.
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
For the reaction:
\(C_{3} H_{8} \left(\right. g \left.\right) + 5 O_{2} \left(\right. g \left.\right) \rightarrow 3 CO_{2} \left(\right. g \left.\right) + 4 H_{2} O \left(\right. l \left.\right)\) at constant temperature, ∆H – ∆E is:
1. | + RT | 2. | – 3RT |
3. | + 3RT | 4. | – RT |
For the given reaction
, the heat of formations of are -188 kJ/mol & -286 KJ/mol respectively. The change in the enthalpy of the reaction will be:
1. – 196 kJ/mol
2. + 196 kJ/mol
3. + 948 kJ/mol
4. – 948 kJ/mol
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. |