For reaction $Ag_2O_{(s)} \to 2Ag_{(s)} + 1/2 O_{2(g)}$,the value of $\Delta H = 30.56 \ kJ \ mol^{-1}$ and $\Delta S = 0.066 \ kJ \ K^{-1} \ mol^{-1}$. Temperature at which free energy change for reaction will be zero,is ............. $K$.

An enthalpy diagram for a particular reaction is given in the figure. Is it possible to decide the spontaneity of a reaction from the given diagram? Explain.

The maximum work (in $kJ \, mol^{-1}$) that can be derived from the complete combustion of $1 \, mole$ of $CO$ at $298 \, K$ and $1 \, atm$ is:
[Standard enthalpy of combustion of $CO = -283.0 \, kJ \, mol^{-1}$; standard molar entropies: $S_{O_2} = 205.1 \, J \, K^{-1} \, mol^{-1}$,$S_{CO} = 197.7 \, J \, K^{-1} \, mol^{-1}$,$S_{CO_2} = 213.7 \, J \, K^{-1} \, mol^{-1}$]

For a particular reversible reaction at temperature $T$,$\Delta H$ and $\Delta S$ were found to be both positive. If $T_e$ is the temperature at equilibrium,the reaction would be spontaneous when

Describe Gibbs energy and spontaneity.

Which of the following conditions are not suitable for a spontaneous reaction?