272367
**Assertion:** $\Delta H$ and $\Delta E$ are almost same for the reaction $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \square \quad 2 \mathrm{NO}(\mathrm{g})$ **Reason:** All reactants and products are gases.
1 If both Assertion and Reason are correct and the Reason is correct explanation of the Assertion.
2 If both Assertion and Reason are correct by Reason is not a correct explanation of the Assertion.
3 If the Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
5 If the Assertion is incorrect but the Reason is correct.
Explanation:
$\Delta \mathrm{H}=\Delta \mathrm{E}+\Delta \mathrm{nRT}$ If there is no change in the moles of reactants (gaseous) and products (gaseous) $\Delta \mathrm{n}=2-(1+1)=0$ $\therefore \Delta \mathrm{H}=\Delta \mathrm{E}$ All reactant and product are gases but this is not reason for $\Delta H=\Delta \mathrm{E}$.
AIIMS-2003
Thermodynamics
272371
**Assertion:** Many endothermic reactions that are not spontaneous at room temperature become at high temperature. **Reason:** Entropy of the system increase with increase in temperature.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}$ $\Delta \mathrm{H}$ is +ve for endothermic process For spontaneous process $\Delta \mathrm{G}<0$ $\therefore \Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}<0$ i.e. $\Delta \mathrm{H}<\mathrm{TS}$ $\Delta \mathrm{G}=0 \mathrm{At}$ equilibrium Entropy of the system also increases with increase in temperature but only slightly.
AIIMS-2012
Thermodynamics
272372
**Assertion :** For an isothermal reversible process $Q=-W$ i.e. work done by the system equals to the heat absorbed by the system. **Reason:** Enthalpy change $(\Delta H)$ is zero for isothermal process.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
For an isothermal process change in internal energy $(\Delta \mathrm{E}$ ) is zero (as it is a function of temperature). According to first law of thermodynamics $\mathrm{Q}+\mathrm{W}=\Delta \mathrm{E}$ Hence, $Q=-W \quad$ (if $\Delta \mathrm{E}=0$ ) If a system undergoes a change in which internal energy of the system remains constant (i.e. $\Delta \mathrm{E}=0$ ) then $-\mathrm{W}=$ Q. This mean that work done by the system is equal to the heat absorbed by the system.
272367
**Assertion:** $\Delta H$ and $\Delta E$ are almost same for the reaction $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \square \quad 2 \mathrm{NO}(\mathrm{g})$ **Reason:** All reactants and products are gases.
1 If both Assertion and Reason are correct and the Reason is correct explanation of the Assertion.
2 If both Assertion and Reason are correct by Reason is not a correct explanation of the Assertion.
3 If the Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
5 If the Assertion is incorrect but the Reason is correct.
Explanation:
$\Delta \mathrm{H}=\Delta \mathrm{E}+\Delta \mathrm{nRT}$ If there is no change in the moles of reactants (gaseous) and products (gaseous) $\Delta \mathrm{n}=2-(1+1)=0$ $\therefore \Delta \mathrm{H}=\Delta \mathrm{E}$ All reactant and product are gases but this is not reason for $\Delta H=\Delta \mathrm{E}$.
AIIMS-2003
Thermodynamics
272371
**Assertion:** Many endothermic reactions that are not spontaneous at room temperature become at high temperature. **Reason:** Entropy of the system increase with increase in temperature.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}$ $\Delta \mathrm{H}$ is +ve for endothermic process For spontaneous process $\Delta \mathrm{G}<0$ $\therefore \Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}<0$ i.e. $\Delta \mathrm{H}<\mathrm{TS}$ $\Delta \mathrm{G}=0 \mathrm{At}$ equilibrium Entropy of the system also increases with increase in temperature but only slightly.
AIIMS-2012
Thermodynamics
272372
**Assertion :** For an isothermal reversible process $Q=-W$ i.e. work done by the system equals to the heat absorbed by the system. **Reason:** Enthalpy change $(\Delta H)$ is zero for isothermal process.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
For an isothermal process change in internal energy $(\Delta \mathrm{E}$ ) is zero (as it is a function of temperature). According to first law of thermodynamics $\mathrm{Q}+\mathrm{W}=\Delta \mathrm{E}$ Hence, $Q=-W \quad$ (if $\Delta \mathrm{E}=0$ ) If a system undergoes a change in which internal energy of the system remains constant (i.e. $\Delta \mathrm{E}=0$ ) then $-\mathrm{W}=$ Q. This mean that work done by the system is equal to the heat absorbed by the system.
272367
**Assertion:** $\Delta H$ and $\Delta E$ are almost same for the reaction $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \square \quad 2 \mathrm{NO}(\mathrm{g})$ **Reason:** All reactants and products are gases.
1 If both Assertion and Reason are correct and the Reason is correct explanation of the Assertion.
2 If both Assertion and Reason are correct by Reason is not a correct explanation of the Assertion.
3 If the Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
5 If the Assertion is incorrect but the Reason is correct.
Explanation:
$\Delta \mathrm{H}=\Delta \mathrm{E}+\Delta \mathrm{nRT}$ If there is no change in the moles of reactants (gaseous) and products (gaseous) $\Delta \mathrm{n}=2-(1+1)=0$ $\therefore \Delta \mathrm{H}=\Delta \mathrm{E}$ All reactant and product are gases but this is not reason for $\Delta H=\Delta \mathrm{E}$.
AIIMS-2003
Thermodynamics
272371
**Assertion:** Many endothermic reactions that are not spontaneous at room temperature become at high temperature. **Reason:** Entropy of the system increase with increase in temperature.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}$ $\Delta \mathrm{H}$ is +ve for endothermic process For spontaneous process $\Delta \mathrm{G}<0$ $\therefore \Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}<0$ i.e. $\Delta \mathrm{H}<\mathrm{TS}$ $\Delta \mathrm{G}=0 \mathrm{At}$ equilibrium Entropy of the system also increases with increase in temperature but only slightly.
AIIMS-2012
Thermodynamics
272372
**Assertion :** For an isothermal reversible process $Q=-W$ i.e. work done by the system equals to the heat absorbed by the system. **Reason:** Enthalpy change $(\Delta H)$ is zero for isothermal process.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
For an isothermal process change in internal energy $(\Delta \mathrm{E}$ ) is zero (as it is a function of temperature). According to first law of thermodynamics $\mathrm{Q}+\mathrm{W}=\Delta \mathrm{E}$ Hence, $Q=-W \quad$ (if $\Delta \mathrm{E}=0$ ) If a system undergoes a change in which internal energy of the system remains constant (i.e. $\Delta \mathrm{E}=0$ ) then $-\mathrm{W}=$ Q. This mean that work done by the system is equal to the heat absorbed by the system.
272367
**Assertion:** $\Delta H$ and $\Delta E$ are almost same for the reaction $\mathrm{N}_2(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \square \quad 2 \mathrm{NO}(\mathrm{g})$ **Reason:** All reactants and products are gases.
1 If both Assertion and Reason are correct and the Reason is correct explanation of the Assertion.
2 If both Assertion and Reason are correct by Reason is not a correct explanation of the Assertion.
3 If the Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
5 If the Assertion is incorrect but the Reason is correct.
Explanation:
$\Delta \mathrm{H}=\Delta \mathrm{E}+\Delta \mathrm{nRT}$ If there is no change in the moles of reactants (gaseous) and products (gaseous) $\Delta \mathrm{n}=2-(1+1)=0$ $\therefore \Delta \mathrm{H}=\Delta \mathrm{E}$ All reactant and product are gases but this is not reason for $\Delta H=\Delta \mathrm{E}$.
AIIMS-2003
Thermodynamics
272371
**Assertion:** Many endothermic reactions that are not spontaneous at room temperature become at high temperature. **Reason:** Entropy of the system increase with increase in temperature.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
$\Delta \mathrm{G}=\Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}$ $\Delta \mathrm{H}$ is +ve for endothermic process For spontaneous process $\Delta \mathrm{G}<0$ $\therefore \Delta \mathrm{H}-\mathrm{T} \Delta \mathrm{S}<0$ i.e. $\Delta \mathrm{H}<\mathrm{TS}$ $\Delta \mathrm{G}=0 \mathrm{At}$ equilibrium Entropy of the system also increases with increase in temperature but only slightly.
AIIMS-2012
Thermodynamics
272372
**Assertion :** For an isothermal reversible process $Q=-W$ i.e. work done by the system equals to the heat absorbed by the system. **Reason:** Enthalpy change $(\Delta H)$ is zero for isothermal process.
1 If both Assertion and Reason are correct and the Reason is the correct explanation of Assertion.
2 If both Assertion and Reason are correct, but Reason is not the correct explanation of Assertion.
3 If Assertion is correct but Reason is incorrect.
4 If both the Assertion and Reason are incorrect.
Explanation:
For an isothermal process change in internal energy $(\Delta \mathrm{E}$ ) is zero (as it is a function of temperature). According to first law of thermodynamics $\mathrm{Q}+\mathrm{W}=\Delta \mathrm{E}$ Hence, $Q=-W \quad$ (if $\Delta \mathrm{E}=0$ ) If a system undergoes a change in which internal energy of the system remains constant (i.e. $\Delta \mathrm{E}=0$ ) then $-\mathrm{W}=$ Q. This mean that work done by the system is equal to the heat absorbed by the system.