For a reaction at $25 \, ^oC$,the enthalpy change and entropy change are $-11.7 \times 10^3 \, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} \, K^{-1}$ respectively. What is the Gibbs free energy in $kJ$?
- A$15.05$
- B$19.59$
- C$2.55$
- D$22.55$
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View SolutionIdentify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.
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View SolutionWhat is the nature of the reaction at $298 \ K$,if the entropy change and enthalpy change for a chemical reaction are $7.4 \ cal \ K^{-1}$ and $-2.5 \times 10^3 \ cal$,respectively?
For a chemical reaction,if $\Delta H = \Delta S > 0$,then $\Delta H = $ ................
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View SolutionData given for the following reaction is as follows:
$FeO_{(s)} + C_{(\text{graphite})} \longrightarrow Fe_{(s)} + CO_{(g)}$
Substance
$\Delta H^{\circ} \text{ (kJ mol}^{-1})$
$\Delta S^{\circ} \text{ (J mol}^{-1} \text{ K}^{-1})$
$FeO_{(s)}$
$-266.3$
$57.49$
$C_{(\text{graphite})}$
$0$
$5.74$
$Fe_{(s)}$
$0$
$27.28$
$CO_{(g)}$
$-110.5$
$197.6$
The minimum temperature in $K$ at which the reaction becomes spontaneous is ....... .
(Integer answer)
$FeO_{(s)} + C_{(\text{graphite})} \longrightarrow Fe_{(s)} + CO_{(g)}$
| Substance | $\Delta H^{\circ} \text{ (kJ mol}^{-1})$ | $\Delta S^{\circ} \text{ (J mol}^{-1} \text{ K}^{-1})$ |
| $FeO_{(s)}$ | $-266.3$ | $57.49$ |
| $C_{(\text{graphite})}$ | $0$ | $5.74$ |
| $Fe_{(s)}$ | $0$ | $27.28$ |
| $CO_{(g)}$ | $-110.5$ | $197.6$ |
The minimum temperature in $K$ at which the reaction becomes spontaneous is ....... .
(Integer answer)
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