The correct thermodynamic conditions for a spontaneous reaction at all temperatures are:
- A$\Delta H > 0$ and $\Delta S < 0$
- B$\Delta H < 0$ and $\Delta S < 0$
- C$\Delta H < 0$ and $\Delta S = 0$
- D$\Delta H < 0$ and $\Delta S > 0$
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For independent processes at $300 \ K$,determine the number of non-spontaneous processes from the following table:
Process $\Delta H \ (kJ \ mol^{-1})$ $\Delta S \ (J \ K^{-1} \ mol^{-1})$ $A$ $-25$ $-80$ $B$ $-22$ $40$ $C$ $25$ $-50$ $D$ $22$ $20$
| Process | $\Delta H \ (kJ \ mol^{-1})$ | $\Delta S \ (J \ K^{-1} \ mol^{-1})$ |
|---|---|---|
| $A$ | $-25$ | $-80$ |
| $B$ | $-22$ | $40$ |
| $C$ | $25$ | $-50$ |
| $D$ | $22$ | $20$ |
For a reaction at $25\,^oC$,the enthalpy change $(\Delta H)$ and entropy change $(\Delta S)$ are $-11.7 \times 10^3\, J \, mol^{-1}$ and $-105 \, J \, mol^{-1} K^{-1}$ respectively. The reaction is:
Medium
View SolutionFor a chemical reaction,if $\Delta H > 0$ and $\Delta S > 0$,under what condition will the reaction not be spontaneous?
Medium
View SolutionAt $273 \ K$ the maximum work done when pressure on $10 \ g$ of hydrogen is reduced from $10 \ atm$ to $1 \ atm$ under isothermal,reversible conditions is (Assume the gas behaves ideally) $(R=8.3 \ J \ K^{-1} \ mol^{-1})$
Identify from the following the correct set of thermodynamic conditions for the reaction to be spontaneous at all temperatures.
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