Thermodynamics Quiz-1

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

4.48 L of an ideal gas at NTP requires 12.0 calories to raise its temperature by $15^\circ C$ at constant volume. The $C_P$ of the gas is

Certain reaction is at equilibrium at $82^\circ C$ and the enthalpy change for this reaction is 21.3 kJ. The value of $\Delta S$(in $JK^{-1}mol^{-1}$) 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?

$\Delta G^\circ$ for a reaction is 46.06 kcal/mole, $K_p$ 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 $20^\circ C$. The gas must be

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

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