5 mole of an ideal gas at temp. T are compressed isothermally from 12 atm. To 24 atm. Where, `r=("Work done along reversible process")/("Work done along single step irreversible process")" (Given : ln 2 = 0.7)"`

5 mole of an ideal gas at temp. T are compressed isothermally from 12 atm. To 24 atm. Calculate the value of 10 r. Where, r=("Work done along reversible process")/("Work done along single step irreversible process")" (Given : ln 2 = 0.7)"

Work done during isothermal reversible process is given

Two moles of an ideal gas at 1 atm are compressed to 2 atm at 273 K. The enthalpy change for the process is

A 5 mol sample of an ideal gas is compressed isothermally and irreversible from 1.5 atm to 15 atm at 27^(@)C . Calculate the work done on the gas in calorie unit.

Two moles of an ideal gas at 2 atm and 27^(@)C is compressed isothermally to half of its volume by external pressure of 4 atm. The work doen is

1 mole of an ideal gas undergoes an isothermal reversible expansion form 10 atm to 1 atm at 300 K. What will be the work done ?

1 mole of an ideal gas undergoes an isothermal reversible expansion form 10 atm to 1 atm at 300 K. What will be the work done ?