Which of the following conditions results in a spontaneous chemical reaction?

The process is spontaneous at the given temperature,if

The entropy and enthalpy changes for the reaction $CO_{(g)} + H_2O_{(g)} \rightleftharpoons CO_{2(g)} + H_{2(g)}$ at $300 \ K$ and $1 \ atm$ are respectively $-42.4 \ J \ K^{-1}$ and $-41.2 \ kJ$. The temperature at which the reaction will go in the reverse direction is (in $K$)

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 $...... \ K$.

The essential condition for the feasibility of a reaction is that

The effect of temperature on the spontaneity of reactions is represented as follows:

Condition	Details
$A$. $\Delta H: +, \Delta S: -$	$T$: any $T$,Spontaneity: Non-spontaneous
$B$. $\Delta H: +, \Delta S: +$	$T$: low $T$,Spontaneity: Non-spontaneous
$C$. $\Delta H: -, \Delta S: -$	$T$: low $T$,Spontaneity: Spontaneous
$D$. $\Delta H: -, \Delta S: +$	$T$: any $T$,Spontaneity: Spontaneous

Which of the above conditions are correctly matched?