For a given chemical reaction $A \rightarrow B$ at $300 \ K$,the free energy change is $-49.4 \ kJ \ mol^{-1}$ and the enthalpy of reaction is $51.4 \ kJ \ mol^{-1}$. The entropy change of the reaction is $..... \ J \ K^{-1} \ mol^{-1}$.
- A$336$
- B$390$
- C$460$
- D$551$
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The effect of temperature on the spontaneity of reactions is represented as follows:
Condition Details $A$. $\Delta H: +, \Delta S: -$ $T$: any $T$, Spontaneity: Non-spontaneous $B$. $\Delta H: +, \Delta S: +$ $T$: low $T$, Spontaneity: Non-spontaneous $C$. $\Delta H: -, \Delta S: -$ $T$: low $T$, Spontaneity: Spontaneous $D$. $\Delta H: -, \Delta S: +$ $T$: any $T$, Spontaneity: Spontaneous
Which of the above conditions are correctly matched?
| Condition | Details |
|---|---|
| $A$. $\Delta H: +, \Delta S: -$ | $T$: any $T$, Spontaneity: Non-spontaneous |
| $B$. $\Delta H: +, \Delta S: +$ | $T$: low $T$, Spontaneity: Non-spontaneous |
| $C$. $\Delta H: -, \Delta S: -$ | $T$: low $T$, Spontaneity: Spontaneous |
| $D$. $\Delta H: -, \Delta S: +$ | $T$: any $T$, Spontaneity: Spontaneous |
Which of the above conditions are correctly matched?
The signs of $\Delta_r H^{\circ}$ and $\Delta_r S^{\circ}$ for a reaction to be spontaneous at all temperatures respectively are
For the reaction $A \longrightarrow B$,$\Delta H^{\circ} = 7.5 \, kJ \, mol^{-1}$ and $\Delta S^{\circ} = 25 \, J \, K^{-1} \, mol^{-1}$. The value of $\Delta G^{\circ}$ and the temperature at which the reaction reaches equilibrium are,respectively:
MediumKVPY 2010
View SolutionFor the decomposition reaction of $N_2O_4$,$\Delta H = 58.04 \, kJ$ and $\Delta S = 176.7 \, J/K$. Calculate $\Delta G$ in $kJ$ at $T = 298 \, K$.
Medium
View Solution$A$ reaction,$A + B \rightarrow C + D + q$,is found to have a positive entropy change. The reaction will be:
Easy
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