For a Van der Waals gas, the following equations hold. P = nRT/(V−nb) − a(n/V)2 dU...
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.
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For a Van der Waals gas, the following equations hold. P =
nRT/(V−nb) − a(n/V)2 dU...
I know that my work is correct. I know that delta U is not 0, and...
I know that my work is correct. I know that delta U is not 0,
and delta H is not 0. How do I complete this problem?
For a Van der Waals gas, the following equations hold. P= nRTIV-nb) - a[n/v2 dU = CydT+ a(n/V)2 dv For chlorine gas, Cvm = 25.6 JK-1 mol-t, a = 6.343 bar L2 mol-2, and b = 0.0542 L molt Calculate q, w, AU, and AH, in joules, when one mole of chlorine gas...
The van der Waals equation of state for a real gas is (P+
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
Van der Waals equation of state is (P+(n2a)/V2)(V-nb)=nRT where a and b are temperature-independent parameters that...
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
Van der Waals Constants Gas CH4 CO2 Cl2 NH3 H20 Xe CCIA 02 N2 Kr a...
Van der Waals Constants Gas CH4 CO2 Cl2 NH3 H20 Xe CCIA 02 N2 Kr a b (bar.L2/mol2) (atm-L2/mol)(L/mol) 2.303 2.273 0.0431 3.658 3.610 0.0429 6.343 6.260 0.0542 4.225 4.170 0.0371 5.537 5.465 0.0305 4.192 4.137 0.0516 20.01 19.75 0.1281 1.382 1.363 1.370 1.351 5.121 5.193 1.355 0.0319 0.0387 0.0106 0.0320 0.0395 Ar 1.336 CO 1.472 1.452 4.544 4.481 0.0434 1.370 1.351 0.0387 3.852 3.799 0.0444 5.36 5.29 0.0443 H2S NO N20 NO2 SO2 HF HCI HBr 6.865 6.770 0.0568...
A gas obeys the van der Waals equation with a = 6.69 atm⋅L2 /mol2 and b...
A gas obeys the van der Waals equation with a = 6.69 atm⋅L2 /mol2 and b = 0.057 L/mol. For the gas Cv = 7.00 cal mol-1 deg-1 . What will be ∆U for a process involving the compression of 5 moles of the gas from a volume of 100 liters at 300 K to a volume of 10 liters at 400 K.
The van der Waals Equation for real gases is shown below. (P+ ) (v – nb)...
The van der Waals Equation for real gases is shown below. (P+ ) (v – nb) = nRT In the equation, what assumption we made in the formulation of the Kinetic Molecular Theory of gases for the material-specific constant "a" correct for? O Particle collisions are elastic, so total kinetic energy is conserved The diffusion rate of molecules is indirectly proportional of their molecular weight Gas particles are in constant, random motion Particle volume is negligible
Question 34 of 34 > Use the van der Waals equation of state to calculate the...
Question 34 of 34 > Use the van der Waals equation of state to calculate the pressure of 3.60 mol of Xe at 469 K in a 5.30 L vessel. Use this list of van der Waals constants. 900 Use the ideal gas equation to calculate the pressure under the same conditions. rect ges Van der Waals Constants Acids and Bases Conjugate Strengths Ionization Constants Gas b Indicators (bar L2/mol) (atm L/mol2) (L/mol) Strong Acids/Bases CH4 2.303 2.2730 .0431 Activity...
Problem 3: PV Work for a van der Waals Gas (1 points) The work for a...
Problem 3: PV Work for a van der Waals Gas (1 points) The work for a reversible, isothermal expansion of an ideal gas was found by starting with the expression for reversible work --CP V2 P dV V1 and substituting the ideal gas equation of state for P(V,T), to obtain V2 w = nRT ln VI Find an expression for the work of a reversible, isothermal expansion of a van der Waals gas by starting with the same expression for...
The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas c...
The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas con- stant, and a (L- atm/mol-) and b (L/mol) are material constants. Determine the volume of 1.5 mol of nitrogen (a .39 L2 atm/mol2. b = 0.03913 L/mol) at temperature of 350 K and pressure of 70 atm.
The van der Waals equation...
2) Suppose that N2(g) may be described by the van der Waals equation of state. Ten...
2) Suppose that N2(g) may be described by the van der Waals equation of state. Ten moles of N, are isothermally and reversibly expanded from a volume of 1.01 to a volume of 10.02 at 300K. Compute the work done in the process. Is the result larger or smaller than the result obtained if the process involved an ideal gas? For N2(g): a = 1.352 atm dm mol-2; b = 3.87 x 10-2 dm² mol-
I know that my work is correct. I know that delta U is not 0,
and delta H is not 0. How do I complete this problem?
For a Van der Waals gas, the following equations hold. P= nRTIV-nb) - a[n/v2 dU = CydT+ a(n/V)2 dv For chlorine gas, Cvm = 25.6 JK-1 mol-t, a = 6.343 bar L2 mol-2, and b = 0.0542 L molt Calculate q, w, AU, and AH, in joules, when one mole of chlorine gas...
Van der Waals Constants Gas CH4 CO2 Cl2 NH3 H20 Xe CCIA 02 N2 Kr a b (bar.L2/mol2) (atm-L2/mol)(L/mol) 2.303 2.273 0.0431 3.658 3.610 0.0429 6.343 6.260 0.0542 4.225 4.170 0.0371 5.537 5.465 0.0305 4.192 4.137 0.0516 20.01 19.75 0.1281 1.382 1.363 1.370 1.351 5.121 5.193 1.355 0.0319 0.0387 0.0106 0.0320 0.0395 Ar 1.336 CO 1.472 1.452 4.544 4.481 0.0434 1.370 1.351 0.0387 3.852 3.799 0.0444 5.36 5.29 0.0443 H2S NO N20 NO2 SO2 HF HCI HBr 6.865 6.770 0.0568...
The van der Waals Equation for real gases is shown below. (P+ ) (v – nb) = nRT In the equation, what assumption we made in the formulation of the Kinetic Molecular Theory of gases for the material-specific constant "a" correct for? O Particle collisions are elastic, so total kinetic energy is conserved The diffusion rate of molecules is indirectly proportional of their molecular weight Gas particles are in constant, random motion Particle volume is negligible
Question 34 of 34 > Use the van der Waals equation of state to calculate the pressure of 3.60 mol of Xe at 469 K in a 5.30 L vessel. Use this list of van der Waals constants. 900 Use the ideal gas equation to calculate the pressure under the same conditions. rect ges Van der Waals Constants Acids and Bases Conjugate Strengths Ionization Constants Gas b Indicators (bar L2/mol) (atm L/mol2) (L/mol) Strong Acids/Bases CH4 2.303 2.2730 .0431 Activity...
Problem 3: PV Work for a van der Waals Gas (1 points) The work for a reversible, isothermal expansion of an ideal gas was found by starting with the expression for reversible work --CP V2 P dV V1 and substituting the ideal gas equation of state for P(V,T), to obtain V2 w = nRT ln VI Find an expression for the work of a reversible, isothermal expansion of a van der Waals gas by starting with the same expression for...
The van der Waals equation gives a relationship between the pressure p (atm), volume V(L), and temperature T(K) for a real gas: .2 where n is the number of moles, R 0.08206(L atm)(mol K) is the gas con- stant, and a (L- atm/mol-) and b (L/mol) are material constants. Determine the volume of 1.5 mol of nitrogen (a .39 L2 atm/mol2. b = 0.03913 L/mol) at temperature of 350 K and pressure of 70 atm.
The van der Waals equation...
2) Suppose that N2(g) may be described by the van der Waals equation of state. Ten moles of N, are isothermally and reversibly expanded from a volume of 1.01 to a volume of 10.02 at 300K. Compute the work done in the process. Is the result larger or smaller than the result obtained if the process involved an ideal gas? For N2(g): a = 1.352 atm dm mol-2; b = 3.87 x 10-2 dm² mol-
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