3 moles of liquid water at 100\deg C and 1 atm go to the vapor phase at 160\deg C and 0.5 atm. Calculate \Delta H, \ Delta S, \Delta G, and \Delta A for the process. You can consider that the vapor behaves as an ideal gas. Data for water that you might need to solve the problem: Cpm (vap) 9 cal/(mol K); \Delta Hm_(vap) = 9360 cal/mol; S\deg298K Cpmvap 9 cal/(molK); AHmvap=9360 cal/mol; S°298K=16.72 cal/(molK)
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- Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.9. L ks] 4.50 mol of N₂ gas (Cvm = 20.6 J mol-¹ K-¹) is enclosed in a piston-cylinder assembly (closed system) and undergoes the cycle depicted graphically below. Assuming N₂ behaves as an ideal gas, calculate q, w, AU and AH for each segment (in kJ). Label each segment with the type of process. Note: segment 2+3 follows the relationship PV = nRT. P (bar) 1.) 20.0 L 2.) 50.0 L 3.) 5.00 bar T = T₂ = T₂ V (L) 2
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