Calculate Q and w for the isothermal reversible expansion of one mole an ideal gas from an initial pressure of 1.0 bar to a final pressure of 0.1 bar at a constant temperature of 273 K respectively.

Calculate q, W, DeltaU and DeltaH for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 1.0 bar to a final pressure of 0.1 bar at a constant temperature of 273K.

Calculate q, W, DeltaU and DeltaH for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 1.0bar to a final pressure of 0.1bar at a constant temperature of 273K .

Calculate q,w , and DeltaU for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 2.0 bar to a final pressure of 0.2 bar at a constant temperature of 273K .

Calculate q,w , and DeltaU for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 2.0 bar to a final pressure of 0.2 bar at a constant temperature of 273K .

Calculate the Delta H for the isothermal reversible expansion of 1 mole of an ideal gas from initial pressure of 1.0 bar to a final pressure 0.1 bar at a constant temperature at 273K.

Calculate triangleq, W, triangleE for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 1.0 bar to final pressure of 0.1 bar at a constant temperature of 273 K.

The pressure-volume of varies thermodynamic process is shown in graphs: Work is the mole of transference of energy. It has been observed that reversible work done by the system is the maximum obtainable work. w_(rev) gt w_(irr) The works of isothermal and adiabatic processes are different from each other. w_("isothermal reversible") = 2.303 nRT log_(10) ((V_(2))/(V_(1))) = 2.303 nRT log_(10)((P_(2))/(P_(1))) w_("adiabatic reversible") = C_(V) (T_(1)-T_(2)) The q value and work done in isothermal reversible expansion of one mole of an ideal gas from initial pressure of 1 bar to final pressure of 0.1 bar at constant temperature 273K are: