The condition for a reaction to occur spontaneously is
- A$\Delta H$ must be negative
- B$\Delta S$ must be negative
- C$(\Delta H - T \Delta S)$ must be negative
- D$(\Delta H + T \Delta S)$ must be negative
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Similar Questions
Calculate the value of $\Delta G$ for the following reaction at $300 \ K$.
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$
Which of the following is correct?
Medium
View SolutionFor $2 \ mol$ of $He$ (ideal gas),find the work done in a process where it is heated from $200 \ K$ to $400 \ K$ such that the enthalpy of the gas varies as : $H = 10 \ V^2$ (in $R$)
Difficult
View SolutionCalculate $\Delta H^{\circ}$ for a reaction at $298 \ K$ if $\Delta S^{\circ} = 120 \ J \ K^{-1}$ and $\Delta G^{\circ} = 28000 \ J$. (in $kJ$)
The relation between $\Delta G$ and $\Delta H$ is
Easy
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