Calculate the work done if $1 \ mole$ of a certain gas is compressed isothermally and reversibly at $300 \ K$ from an initial pressure $x \ bar$ to a final pressure $2x \ bar$ $[R = 8.314 \ J \ K^{-1} \ mol^{-1}]$. (in $kJ$)

Data given for the following reaction is as follows:
$FeO_{(s)} + C_{(\text{graphite})} \longrightarrow Fe_{(s)} + CO_{(g)}$

Substance	$\Delta H^{\circ} \text{ (kJ mol}^{-1})$	$\Delta S^{\circ} \text{ (J mol}^{-1} \text{ K}^{-1})$
$FeO_{(s)}$	$-266.3$	$57.49$
$C_{(\text{graphite})}$	$0$	$5.74$
$Fe_{(s)}$	$0$	$27.28$
$CO_{(g)}$	$-110.5$	$197.6$

The minimum temperature in $K$ at which the reaction becomes spontaneous is ....... .
(Integer answer)

The standard entropy change for the reaction $4 Fe ( s ) + 3 O_{2} ( g ) \rightarrow 2 Fe_{2} O_{3} ( s )$ is $-550 \ J K^{-1}$ at $298 \ K$. Given: The standard enthalpy change for the reaction is $-165 \ kJ \ mol^{-1}$. The temperature in $K$ at which the reaction attains equilibrium is ... . (Nearest Integer)

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

Identify the correct statement for the change in Gibbs energy $(\Delta G_{\text{system}})$ for a system at constant temperature and pressure.

For a spontaneous process,which of the following conditions is most favorable?