The work done when 1 mole of gas expands reversibly and isothermally from a pressure of 5 atm to 1 atm at 300 K is: ​
(Given log 5 = 0.6989 and R = 8.314 J K^-1 mol^-1)
1. zero J
2. 150 J
3. +4014.6 J
4. -4014.6 J

An ideal gas expands isothermally from ${10}^{-3}{m}^3 to {10}^{-2} m^3$ at 300 K against a constant pressure of ${10}^5 N{m}^{-2}$. The work done by  the gas is:

A gas is allowed to expand in a well-insulated container against a constant external pressure of 2.5atm from an initial volume of 2.50 L to a final volume of 4.50L. The change in internal energy U of the gas in joules will be:
1. –500J
2. –505J
3. –506J
4. –508J

Identify which of the following is the correct option for free expansion of an ideal gas under adiabatic condition.

1.  $\mathrm{ \Delta q}\ne 0,$ $∆\mathrm{T}=0,$ $\mathrm{W}=0$
2.  $\mathrm{ \Delta q}=0,$ $∆\mathrm{T}=0,$ $\mathrm{W}=0$
3.  $\mathrm{ \Delta q}=0,$ $∆\mathrm{T}<0,$ $\mathrm{W}\ne 0$
4.  $\mathrm{ \Delta q}=0,$ $∆\mathrm{T}\ne 0,$ $\mathrm{W}=0$

Three moles of an ideal gas expanded spontaneously into vacuum. The work done will be:

1. 3 Joules

2. 9 Joules

3. Zero

4. Infinite

The work done during the expansion of a gas from a volume of 4 dm³ to 6 dm³ against a constant external pressure of 3 atm is:

1. –608 J

2. +304 J

3. –304 J

4. –6 J 

The molar heat capacity of water at constant pressure, C, is 75 JK^–1 mol^–1. When 1.0 kJ of heat is supplied to 100 g of water which is free to expand, the increase in temperature of the water is: