Which of the following is not correct?
- A$\Delta G$ is negative for a spontaneous reaction
- B$\Delta G$ is positive for a spontaneous reaction
- C$\Delta G$ is zero for a reversible reaction
- D$\Delta G$ is positive for a non-spontaneous reaction
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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.
Calculate the value of $\Delta G$ for the following reaction at $300 \ K$.
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$
For the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ at $373 \ K$ and $1 \ atm$ pressure,which of the following is true?
Medium
View SolutionUnder isothermal and reversible conditions,the term "free energy" in thermodynamics signifies
The values of $\Delta H$ and $\Delta S$ of a certain reaction are $-400 \text{ kJ mol}^{-1}$ and $-20 \text{ kJ mol}^{-1} \text{ K}^{-1}$ respectively. The temperature below which the reaction is spontaneous, is
MediumWBJEE 2014
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