In which of the following conditions will a reaction always be spontaneous at all temperatures?
- A$\Delta H = +ve, \Delta S = +ve$
- B$\Delta H = +ve, \Delta S = -ve$
- C$\Delta H = -ve, \Delta S = -ve$
- D$\Delta H = -ve, \Delta S = +ve$
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Calculate the work done if $1 \ mole$ of an ideal gas is compressed isothermally and reversibly from $12 \ dm^3$ to $6 \ dm^3$ at $300 \ K$. $\left[R = 8.314 \ J \ K^{-1} \ mol^{-1}\right]$ (in $kJ$)
Based on the provided table,which of the following options correctly identifies the spontaneous reactions?
$\Delta_r H^{\circ}$ $\Delta_r S^{\circ}$ $\Delta_r G^{\circ}$ Spontaneity of the reaction $A$ $+$ $+$ $+$ Spontaneous at low $T$ $B$ $+$ $+$ $-$ Spontaneous at high $T$ $C$ $-$ $-$ $-$ Spontaneous at low $T$ $D$ $+$ $-$ $+$ Spontaneous at high $T$
| $\Delta_r H^{\circ}$ | $\Delta_r S^{\circ}$ | $\Delta_r G^{\circ}$ | Spontaneity of the reaction | |
|---|---|---|---|---|
| $A$ | $+$ | $+$ | $+$ | Spontaneous at low $T$ |
| $B$ | $+$ | $+$ | $-$ | Spontaneous at high $T$ |
| $C$ | $-$ | $-$ | $-$ | Spontaneous at low $T$ |
| $D$ | $+$ | $-$ | $+$ | Spontaneous at high $T$ |
The condition of spontaneity of a process is
Describe Gibbs energy and spontaneity.
Medium
View SolutionWhich of the following pairs of a chemical reaction is certain to result in a spontaneous reaction?
MediumAIPMT 2005
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