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?

The dependence of Gibbs free energy on pressure for an isothermal process of an ideal gas is given by:

$2 \, mol$ of zinc is dissolved in $HCl$ at $25 \, ^\circ C$. The work done in an open vessel is: (in $, kJ$)

Calculate $\Delta H^{\circ}$ for a reaction at $298 \ K$ if $\Delta S^{\circ} = 120 \ J \ K^{-1}$ and $\Delta G^{\circ} = 28000 \ J$. (in $kJ$)

$A$ $4.50 \ g$ sample of methane occupies $12.7 \ L$ at $310 \ K$. Calculate the work done in $J$ when the gas undergoes isothermal expansion against a constant external pressure of $200 \ torr$ until the volume increases by $3.3 \ L$. (in $.99$)

The boiling point of water at $1 \ atm$ is $100^{\circ} C$. Which among the following is true for vaporisation of water at $75^{\circ} C$?