How many calories are required to heat 40 gram of argon from $40^{\circ }40^\backslash circ$ to $100^{\circ }C100^\backslash circ\; C$ at constant volume? (R = 2 ${\text{cal K}}^{-1}{\text{mol}}^{-1}\backslash text\{cal\; K\}^\{-1\}\backslash text\{mol\}^\{-1\}$ )

4.48 L of an ideal gas at NTP requires 12.0 calories to raise its temperature by $15^{\circ }C15^\backslash circ\; C$ at constant volume. The $C_{P}C\_P$ of the gas is

Certain reaction is at equilibrium at $82^{\circ }C82^\backslash circ\; C$ and the enthalpy change for this reaction is 21.3 kJ. The value of $\mathrm{\Delta }S\backslash Delta\; S$(in $J{K}^{-1}mo{l}^{-1}JK^\{-1\}mol^\{-1\}$) for the reaction is

Which of the following thermodynamic relation is correct?

A reaction is spontaneous at low temperature but non-spontaneous at high temperature. Which of the following is true for the reaction?

$\mathrm{\Delta }{G}^{\circ }\backslash Delta\; G^\backslash circ$ for a reaction is 46.06 kcal/mole, $K_{p}K\_p$ for the reaction at 300 K is

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The enthalpy change (in kJ) for the process is

When 0.1 mole of a gas absorbs 41.75 J of heat at constant volume, the rise in temperature occurs equal to $20^{\circ }C20^\backslash circ\; C$. The gas must be

One mole of an ideal gas expands freely and isothermally at 300 K from 10 litres to 100 litres. If $\mathrm{\Delta }U=0\backslash Delta\; U\; =\; 0$, the value of $\mathrm{\Delta }H\backslash Delta\; H$ is

When 100 g of water is electrolysed at constant pressure of 1 atm and temperature of $25^{\circ }C25^\backslash circ\; C$, the work of expansion is