

2. Derive an expression for (as) for a gas with the equation of state: P(V-nB) = nRT, where B is a constant. 2. De...
Van der Waals equation of state is (P+(n2a)/V2)(V-nb)=nRT where a and b are temperature-independent parameters that have different values for each gas. For CO2, a=0.3640 Pa m6/mol2 and b=4.267*10-5 m3/mol a) Write this equation as a cubic equation in V
3. A gas obeys the equation of state PV = nRT - an'/V, where n is the number of moles of gas and a is constant. Substitute with rearrangement into the differential equation for work, and integrate from Vito V2 to find an equation for the work done by this gas as the result of a reversible isothermal process. Show algebraically that the work is proportional to n to the first power.
3. A gas obeys the equation of state PV = nRT - an'/V, where n is the number of moles of gas and a is constant. Substitute with rearrangement into the differential equation for work, and integrate from Vito V2 to find an equation for the work done by this gas as the result of a reversible isothermal process. Show algebraically that the work is proportional to n to the first power.
10. A nonideal gas obeys the equation of state PV = nRT - api where a is a positive constant. Obtain an expression for the Joule-Thomson coefficient for this gas in terms of the constant a and the heat capacity of the gas. Does the temperature of the gas increase or decrease in a Joule-Thomson experiment? Coorry?
8. 10 Point Bonus! The Ideal Gas Equation of State is pV = nRT, where n= number of moles of gas & R is the ideal the gas constant. The Van der Waals Equation of State is briefly discussed in Ch. 5 of the book by Reif. It is an empirical, crude attempt to improve on the Ideal Gas Model by allowing gas molecules to interact with each other. For one mole of non-ideal gas this equation of state is...
The Ideal Gas Law is given by the equation:pv=nrt Where: p = pressure v = volume n = moles t = temperature in Kelvin In order to solve for the volume, V, you must multiply both sides of the equation by the same expression: PV x ___=nRT X __ The resulting equation is: V=? In order to solve the equation above for , you must multiply both sides of the equation by the same expression: a=b/c ax_?_=b/c x _?_ The...
IGL: PV = nRT VdW: ( P + an2/V2 )( V – nb ) = nRT where a and b are constants specific to the gas. 1.) CO2 behaves likes a Van der Waals gas with constants a = 0.364 J.m3/mol2 and b = .000043 m3/mol. If 2.5 moles of CO2 is put in a cubical tank (each side is 10cm) at 400K, what would be the pressure? What would be the force the gas exerts on each face of...
For a Van der Waals gas, the following equations hold. P = nRT/(V−nb) − a(n/V)2 dU = CV dT + a(n/V)2 dV For chlorine gas, CV,m = 25.6 J K−1 mol−1, a = 6.343 bar L2 mol−2, and b = 0.0542 L mol−1. Calculate q, w, ΔU, and ΔH, in joules, when one mole of chlorine gas is expanded isothermally and reversibly at 449 K from 7.0 L to 15.0 L.
An equation of state for a system is determined to be given by the following: P^(3/4)*(V - nb) = nRT Show that the expansivity, B, is given by the following: B = (V - nb) / (TV)
The van der Waals equation of state for a real gas is (P+ ) (V - nb) = nRT At what pressure will 1.00 mole of CH4 be in a 10.0 L container at 298 K assuming CH4 is a real gas. (van der Waals constants for CH4 are α = -2.253 L2 atm mol-2. b = 0.04278 L mol-1) 2.43 atm 2.28 atm 2.51 atm 24.5 atm 0.440 atm