At constant pressure and temperature,the direction of any spontaneous chemical reaction is towards the state where there is a decrease in

What is the free energy change $\Delta G$ when $1.0 \ mole$ of water at $100 \ ^oC$ and $1 \ atm$ pressure is converted into steam at $100 \ ^oC$ and $1 \ atm$ pressure?

The standard enthalpy and standard entropy of decomposition of $N_2O_4$ to $NO_2$ are $55.0 \ kJ \ mol^{-1}$ and $175.0 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard free energy change for this reaction at $25 ^{\circ}C$ in $J \ mol^{-1}$ is $............$ $(Nearest \ integer)$.

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

Calculate the value of $\Delta G$ for the following reaction at $300 \ K$.
$H_2O_{(s)} \longrightarrow H_2O_{(l)}$
$(\Delta H = 7 \ kJ, \Delta S = 24.8 \ J \ K^{-1})$

$\Delta H$ and $\Delta S$ for a reaction are $+30.0 \ kJ \ mol^{-1}$ and $0.06 \ kJ \ K^{-1} \ mol^{-1}$ at $1 \ atm$ pressure. The temperature at which free energy change is equal to zero and the nature of the reaction below this temperature are: