272726 Work done by 1 mole of an ideal gas for its adiabatic reversible change when temperature attains $T_2$ from $T_1$ is'

272654 The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of $1 \mathrm{~L}$ to $10 \mathrm{~L}$ at $300 \mathrm{~K}$ is
$\left(\mathrm{R}=0.0083 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

272658 Work done by an ideal gas at a constant volume is ......... .

272659 A system undergoes a process in which $\Delta \mathrm{U}=+300 \mathrm{~J}$ while absorbing $400 \mathrm{~J}$ of heat energy and undergoing an expansion against 0.5 bar. What is the change in volume (in L)?

272661 One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at $300 \mathrm{~K}$. $\Delta \mathrm{u}, \mathrm{q}$ and work done in the process are $\left[\mathrm{R}=8.3 \times 10^{-3} \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$

272726 Work done by 1 mole of an ideal gas for its adiabatic reversible change when temperature attains $T_2$ from $T_1$ is'

272654 The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of $1 \mathrm{~L}$ to $10 \mathrm{~L}$ at $300 \mathrm{~K}$ is
$\left(\mathrm{R}=0.0083 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

272658 Work done by an ideal gas at a constant volume is ......... .

272659 A system undergoes a process in which $\Delta \mathrm{U}=+300 \mathrm{~J}$ while absorbing $400 \mathrm{~J}$ of heat energy and undergoing an expansion against 0.5 bar. What is the change in volume (in L)?

272661 One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at $300 \mathrm{~K}$. $\Delta \mathrm{u}, \mathrm{q}$ and work done in the process are $\left[\mathrm{R}=8.3 \times 10^{-3} \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$

272726 Work done by 1 mole of an ideal gas for its adiabatic reversible change when temperature attains $T_2$ from $T_1$ is'

272654 The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of $1 \mathrm{~L}$ to $10 \mathrm{~L}$ at $300 \mathrm{~K}$ is
$\left(\mathrm{R}=0.0083 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

272658 Work done by an ideal gas at a constant volume is ......... .

272659 A system undergoes a process in which $\Delta \mathrm{U}=+300 \mathrm{~J}$ while absorbing $400 \mathrm{~J}$ of heat energy and undergoing an expansion against 0.5 bar. What is the change in volume (in L)?

272661 One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at $300 \mathrm{~K}$. $\Delta \mathrm{u}, \mathrm{q}$ and work done in the process are $\left[\mathrm{R}=8.3 \times 10^{-3} \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$

272726 Work done by 1 mole of an ideal gas for its adiabatic reversible change when temperature attains $T_2$ from $T_1$ is'

272654 The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of $1 \mathrm{~L}$ to $10 \mathrm{~L}$ at $300 \mathrm{~K}$ is
$\left(\mathrm{R}=0.0083 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

272658 Work done by an ideal gas at a constant volume is ......... .

272659 A system undergoes a process in which $\Delta \mathrm{U}=+300 \mathrm{~J}$ while absorbing $400 \mathrm{~J}$ of heat energy and undergoing an expansion against 0.5 bar. What is the change in volume (in L)?

272661 One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at $300 \mathrm{~K}$. $\Delta \mathrm{u}, \mathrm{q}$ and work done in the process are $\left[\mathrm{R}=8.3 \times 10^{-3} \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$

272726 Work done by 1 mole of an ideal gas for its adiabatic reversible change when temperature attains $T_2$ from $T_1$ is'

272654 The work done when 2 moles of an ideal gas expands reversibly and isothermally from a volume of $1 \mathrm{~L}$ to $10 \mathrm{~L}$ at $300 \mathrm{~K}$ is
$\left(\mathrm{R}=0.0083 \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

272658 Work done by an ideal gas at a constant volume is ......... .

272659 A system undergoes a process in which $\Delta \mathrm{U}=+300 \mathrm{~J}$ while absorbing $400 \mathrm{~J}$ of heat energy and undergoing an expansion against 0.5 bar. What is the change in volume (in L)?

272661 One mole of a perfect gas expands isothermally and reversibly from $10 \mathrm{dm}^3$ to $20 \mathrm{dm}^3$ at $300 \mathrm{~K}$. $\Delta \mathrm{u}, \mathrm{q}$ and work done in the process are $\left[\mathrm{R}=8.3 \times 10^{-3} \mathrm{~kJ} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$