Consider an ideal gas that occupies 2.25 L at 1.33 bar. Calculate the work required to compress the gas isothermally to a volume of 1.50 L at a constant pressure of 2.00 bar followed by another isothermal compression to 0.800 L at a constant pressure of 3.75 bar. Compare your result with the work of compressing the gas isothermally and reversibly from 2.25 L to 0.80 L.

Consider work, heat, and internal energy. Explain the molecular basis for each. Which are state and which are path functions? Provide reasoning to support your claims.

Estimate (i.e. calculate approximately) the thermal energy of 1 mole of H20 vapor at room temperature.

Everything needed is included Consider the reversible and isothermal compression of 2.0 moles of ammonia (NH3 (g)) from an initial volume of 10.0 L to a final volume of 1.00 L, at a constant temperature of 298 K: 6a. Calculate the work w and heat q associated with this change in volume, considering NH3 to be an ideal gas. 6b. Calculate the work w (but not the heat) using the virial equation of state, with second virial coefficient B = −0.297 L/mol for NH3 at this temperature (and ignoring any higher coefficients).