The correct thermodynamic conditions for a spontaneous reaction at all temperatures are:

$A$ reaction,$A + B \rightarrow C + D + q$,is found to have a positive entropy change. The reaction will be:

For a reaction to be spontaneous at any temperature,which of the following is true?

Under what conditions will a reaction become spontaneous at all temperatures?

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 the reaction at $298 \ K$,$2 \ A^{+}B \rightarrow C$. $\Delta H = 400 \ kJ \ mol^{-1}$ and $\Delta S = 0.2 \ kJ \ mol^{-1} \ K^{-1}$. The reaction will become spontaneous above $...... \ K$.