For a reaction with $\Delta H = +ve$ and $\Delta S = +ve$,which of the following statements is correct?
- AThe reaction is spontaneous at high temperatures.
- BThe reaction is spontaneous at low temperatures.
- CThe reaction is non-spontaneous at high temperatures.
- DThe reaction is non-spontaneous at all temperatures.
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Similar Questions
Identify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous at all temperatures.
At what temperature $(T \ K)$ will the reaction be in equilibrium (in $K$)? $Ag_2O_{(s)} \rightarrow 2Ag_{(s)} + \frac{1}{2} O_{2(g)}$,given $\Delta H = 30.5 \ kJ \ mol^{-1}$ and $\Delta S = 0.066 \ kJ \ K^{-1} \ mol^{-1}$.
Medium
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)
Compare the following criteria for spontaneity of a reaction based on the values of $\Delta_{\text{r}}H^0$,$\Delta_{\text{r}}S^0$,and $\Delta_{\text{r}}G^0$:
$\Delta_{\text{r}}H^0$ $\Delta_{\text{r}}S^0$ $\Delta_{\text{r}}G^0$ Description $(a) (+)$ $(-)$ $(+)$ $(i) \text{ Non-spontaneous at all temperatures}$ $(b) (-)$ $(-)$ $(-)$ $(ii) \text{ Spontaneous at low temperatures}$ $(c) (-)$ $(+)$ $(-)$ $(iii) \text{ Spontaneous at all temperatures}$
| $\Delta_{\text{r}}H^0$ | $\Delta_{\text{r}}S^0$ | $\Delta_{\text{r}}G^0$ | Description |
|---|---|---|---|
| $(a) (+)$ | $(-)$ | $(+)$ | $(i) \text{ Non-spontaneous at all temperatures}$ |
| $(b) (-)$ | $(-)$ | $(-)$ | $(ii) \text{ Spontaneous at low temperatures}$ |
| $(c) (-)$ | $(+)$ | $(-)$ | $(iii) \text{ Spontaneous at all temperatures}$ |
Medium
View SolutionFor the reaction $Ag_2O_{(s)} \rightarrow 2Ag_{(s)} + 1/2 O_{2_{(g)}}$,the value of $\Delta H = 30.56 \, kJ \, mol^{-1}$ and $\Delta S = 66 \, J \, K^{-1} \, mol^{-1}$. At what temperature $(K)$ will the change in free energy for the reaction be zero?
Medium
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