For the melting of $3 \ mol$ of ice at $0^o \text{C}$,$\Delta G = \dots \dots$

$A$ reaction has both $\Delta H$ and $\Delta S$ negative. The rate of reaction

Calculate the work done when $1 \text{ mole}$ of an ideal gas is expanded reversibly and isothermally from an initial pressure $P_1 = 10 \text{ bar}$ to a final pressure $P_2 = 1 \text{ bar}$ at a constant temperature $T = 300 \text{ K}$. $[R = 8.314 \text{ J K}^{-1} \text{ mol}^{-1}]$ (in $\text{ kJ}$)

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 change,free energy change $\Delta G$ is

$A$ process is taking place at constant temperature and pressure. Then