The relation $\Delta G = \Delta H - T\Delta S$ was given by

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?

State the criteria for a spontaneous process in terms of $\Delta G$ at constant pressure and temperature.

For a spontaneous reaction at all temperatures, which of the following is correct?

For the oxidation of ammonia at $298 \ K$,the standard enthalpy and standard entropy changes are $-382.64 \ kJ \ mol^{-1}$ and $-145.6 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard Gibbs energy change for the same reaction at $298 \ K$ is $..... \ kJ \ mol^{-1}$.

One mole of an ideal gas at $1 \ atm$ pressure is filled in a bulb of $10 \ L$ capacity and is connected to a vacuum bulb of $100 \ L$ capacity. How much work is done in this process in Joules?