369304 In an isothermal reversible expansion of 2 moles of ideal gas at 300 K from 1.10 L to 11.0 L , the maximum work done is ____ kcal.
( \({\mathrm{\left.\mathrm{R}=2 \mathrm{cal} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)}}\)

369305 In adiabatic conditions, 2 moles of \(\mathrm{CO}_{2}\) gas at \(300 \mathrm{~K}\) is expanded such that its volume becomes 27 times. Then, the work done is \(\left(\mathrm{C}_{\mathrm{v}}=6 \mathrm{calmol}^{-1}\right.\) and \(\left.\gamma=1.33\right)\)

369306 One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of \(\mathrm{27^{\circ} \mathrm{C}}\). If the work done during the process is \(\mathrm{3 \mathrm{~kJ}}\), the final temperature will be equal to \(\mathrm{\left(\mathrm{C}_{V}=20 \mathrm{~J} \mathrm{~K}^{-1}\right)}\)

369307 The change in internal energy of a system when no heat is absorbed by the system from the surroundings, but work \(\mathrm{(\mathrm{w})}\) is done on the system is

369308 In a process, \(\mathrm{701 \mathrm{~J}}\) of heat is absorbed by a system and \(\mathrm{394 \mathrm{~J}}\) of work is done by the system. The change in internal energy for the process is

369304 In an isothermal reversible expansion of 2 moles of ideal gas at 300 K from 1.10 L to 11.0 L , the maximum work done is ____ kcal.
( \({\mathrm{\left.\mathrm{R}=2 \mathrm{cal} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)}}\)

369305 In adiabatic conditions, 2 moles of \(\mathrm{CO}_{2}\) gas at \(300 \mathrm{~K}\) is expanded such that its volume becomes 27 times. Then, the work done is \(\left(\mathrm{C}_{\mathrm{v}}=6 \mathrm{calmol}^{-1}\right.\) and \(\left.\gamma=1.33\right)\)

369306 One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of \(\mathrm{27^{\circ} \mathrm{C}}\). If the work done during the process is \(\mathrm{3 \mathrm{~kJ}}\), the final temperature will be equal to \(\mathrm{\left(\mathrm{C}_{V}=20 \mathrm{~J} \mathrm{~K}^{-1}\right)}\)

369307 The change in internal energy of a system when no heat is absorbed by the system from the surroundings, but work \(\mathrm{(\mathrm{w})}\) is done on the system is

369308 In a process, \(\mathrm{701 \mathrm{~J}}\) of heat is absorbed by a system and \(\mathrm{394 \mathrm{~J}}\) of work is done by the system. The change in internal energy for the process is

369304 In an isothermal reversible expansion of 2 moles of ideal gas at 300 K from 1.10 L to 11.0 L , the maximum work done is ____ kcal.
( \({\mathrm{\left.\mathrm{R}=2 \mathrm{cal} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)}}\)

369305 In adiabatic conditions, 2 moles of \(\mathrm{CO}_{2}\) gas at \(300 \mathrm{~K}\) is expanded such that its volume becomes 27 times. Then, the work done is \(\left(\mathrm{C}_{\mathrm{v}}=6 \mathrm{calmol}^{-1}\right.\) and \(\left.\gamma=1.33\right)\)

369306 One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of \(\mathrm{27^{\circ} \mathrm{C}}\). If the work done during the process is \(\mathrm{3 \mathrm{~kJ}}\), the final temperature will be equal to \(\mathrm{\left(\mathrm{C}_{V}=20 \mathrm{~J} \mathrm{~K}^{-1}\right)}\)

369307 The change in internal energy of a system when no heat is absorbed by the system from the surroundings, but work \(\mathrm{(\mathrm{w})}\) is done on the system is

369308 In a process, \(\mathrm{701 \mathrm{~J}}\) of heat is absorbed by a system and \(\mathrm{394 \mathrm{~J}}\) of work is done by the system. The change in internal energy for the process is

369304 In an isothermal reversible expansion of 2 moles of ideal gas at 300 K from 1.10 L to 11.0 L , the maximum work done is ____ kcal.
( \({\mathrm{\left.\mathrm{R}=2 \mathrm{cal} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)}}\)

369305 In adiabatic conditions, 2 moles of \(\mathrm{CO}_{2}\) gas at \(300 \mathrm{~K}\) is expanded such that its volume becomes 27 times. Then, the work done is \(\left(\mathrm{C}_{\mathrm{v}}=6 \mathrm{calmol}^{-1}\right.\) and \(\left.\gamma=1.33\right)\)

369306 One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of \(\mathrm{27^{\circ} \mathrm{C}}\). If the work done during the process is \(\mathrm{3 \mathrm{~kJ}}\), the final temperature will be equal to \(\mathrm{\left(\mathrm{C}_{V}=20 \mathrm{~J} \mathrm{~K}^{-1}\right)}\)

369307 The change in internal energy of a system when no heat is absorbed by the system from the surroundings, but work \(\mathrm{(\mathrm{w})}\) is done on the system is

369308 In a process, \(\mathrm{701 \mathrm{~J}}\) of heat is absorbed by a system and \(\mathrm{394 \mathrm{~J}}\) of work is done by the system. The change in internal energy for the process is

369304 In an isothermal reversible expansion of 2 moles of ideal gas at 300 K from 1.10 L to 11.0 L , the maximum work done is ____ kcal.
( \({\mathrm{\left.\mathrm{R}=2 \mathrm{cal} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)}}\)

369305 In adiabatic conditions, 2 moles of \(\mathrm{CO}_{2}\) gas at \(300 \mathrm{~K}\) is expanded such that its volume becomes 27 times. Then, the work done is \(\left(\mathrm{C}_{\mathrm{v}}=6 \mathrm{calmol}^{-1}\right.\) and \(\left.\gamma=1.33\right)\)

369306 One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of \(\mathrm{27^{\circ} \mathrm{C}}\). If the work done during the process is \(\mathrm{3 \mathrm{~kJ}}\), the final temperature will be equal to \(\mathrm{\left(\mathrm{C}_{V}=20 \mathrm{~J} \mathrm{~K}^{-1}\right)}\)

369307 The change in internal energy of a system when no heat is absorbed by the system from the surroundings, but work \(\mathrm{(\mathrm{w})}\) is done on the system is

369308 In a process, \(\mathrm{701 \mathrm{~J}}\) of heat is absorbed by a system and \(\mathrm{394 \mathrm{~J}}\) of work is done by the system. The change in internal energy for the process is