.) 5.00 moles of He ( assumed to be an ideal gas) initially at 300 K and 1.00 bar is compressed isothermally to a final pressure of 4.00 bar. a). Calculate q, w, AU and Delta H if the compression is performed reversibly b). Calculate q, w, AU and Delta*H if the compression is performed irreversibly with a constant 4.00 bar external pressure.

What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?

Asampleof a monatomic ideal gas doubles itsvolume reversibly and adiabatically. By what percentage does its absolute temperature change?

The ideal gas law is theequation of state for an ideal gas. Why cantit be used to determine TpH?

Calculate AS, AStot, and AS sur when the volume of 175 g of CO initially at 273 K and 1.00 bar increases by a factor of three in an adiabatic reversible expansion. Take Cp,m to be constant at the value 29.14 J-mol-¹.K-¹ and assume ideal gas behavior. The temperature of the surroundings is 273 K. Express your answers in joules per kelvin to three significant figures separated by commas. AS, AStot, AS sur = Submit Request Answer Part B IVE ΑΣΦ AS, AStot, AS sur = Calculate AS, AStot, and ASsur when the volume of 175 g of CO initially at 273 K and 1.00 bar increases by a factor of three in an expansion against Pext = 0. Take CP,m to be constant at the value 29.14 J. mol-¹.K-¹ and assume ideal gas behavior. The temperature of the surroundings is 273 K. Express your answers in joules per kelvin to three significant figures separated by commas. IVE ΑΣΦ ? 2 J.K-1 ? J.K-1

4. Determine the values of AHsys, ASys, ASsurr, and ASiot when a 1.75 mol sample of superheated benzene vaporizes at 365.0 K and 1 bar. Assume the temperature of the surroundings stays constant at 365.0 K. Relevant benzene data: CPm.lig=135.7 J-mol--K-; CP.m.gas 108.8 J-mol ''K'; Tvop = 353.3 K at 1 bar; AHvap = 30.72 kJ/mol at 353.3 K and 1 bar. Assume the heat capacities are constant over the relevant temperature ranges. %3D %3D

Given these relation, prove this without usin Maxwell relatios as - ( ), aV ӘT JP/T P

I mol of per feet gas molecules at 27°c is expanded reversibly isothermally from an lnitial pressure o 3.00 atm to final pressure of 1.00 atm, determine the Value 9,W, DEDH, DS, OSur. DS .

For a van der Waals gas: a V2 Calculate AUm (in J mol-) for the isothermal reversible expansion of N2 gas from an initi volume of 1.00 L to 24.8 L at 298 K. (3) [Given: a(N2) = 1.352 L2. atm mol-2]

In this assignment, we will consider 1 mole of N2(g) which is in a closed container. In state 1, the temperature is 25°C and the pressure in the container is 10 bar.We assume that N2  behaves like an ideal gas and that Cp,m(g) = 29.125 J mol-1K-1, and is independent of temperature. 1) How large will a) the volume work, b) the heat and c) the change in enthalpy of N2 be if, starting from state 1, the volume of the container was changed in a reversible and isothermal manner so that the pressure in the container drops to 1 bar? 2) How big will a) the volume work, b) the heat and c) the change in enthalpy of N2 be if, again starting from state 1, the volume of the container was changed in a reversible and adiabatic way so that the pressure in the container drops to 1 bar? 3) a) Explain what reversible means in tasks 1) and 2) b) state what the change in the entropy of the universe is in tasks 1) and 2). 4) How large will a) the volume work, b) the heat and c) the change in enthalpy of N2…