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Calculate the change in chemical potential of a perfect gas when its pressure is increased isothermally from 1.8 atm to 29.5 atm at 40°C
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- At 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 2 B(g) = C(g) + 3 D(g) were found to be PA = 4.41 bar, PB 5.54 bar, Pc = 4.92 bar, and P, = 5.18 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ/molAt 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4 B(g)=2C(g)+D(g) were found to be PA = 4.74 bar, Pg 5.52 bar, Pc = 4.94 bar, and Pp 5.78 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ?In the reaction 2A (g) + B(g)==>2C(g) + D(g), 3.00 mol A was mixed with 2 mol of B and 0.5 mol of D. The system was allowed to come to equilibrium. At equilibrium, 1.2 mol of C was present at a total pressure of 1 bar. Calculate the mole fractions of each species at equilibrium, K, and ΔGr at 298 K.
- At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 2 B(g) = C(g) + 2 D(g) were found to be PA = 4.25 atm, Pg = 5.05 atm, Pc = 4.13 atm, and Pp 4.94 atm. %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ mol1. Assume the molar Gibbs free energy of a gas is given by the equation: Gm - RT In(÷)+ (a + bT)P = 0, where po is the standard pressure and a and b are gas-dependent constants. Derive an equation of state for this gas. Show the final result in the form of PV=?.Calculate ΔS (for the system) when the state of 2.00 mol of gas molecules, for which Cp,m = R, is changed from 25 °C and 1.50 atm to 135 °C and 7.00 atm.
- At 25 °C, the equilibrium partial pressures for the reaction 2A(g)+4B(g)↽−−⇀2C(g)+D(g) were found to be PA=5.86 bar, PB=5.73 bar, PC=4.88 bar, and PD=4.65 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ΔGrxn°= kJ/molAt 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4B(g)2C(g) + D(g) were found to be P = 5.98 bar, P = 4.72 bar, Pe= 5.25 bar, and P = 4.16 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? AGOR= kJ/molEstimate the enthalpy of vaporization of water at 100 °c from its value at 25 °c, 44.01 kJ mol-1, given the constant pressure molar heat capacities of 75.29 J K-1 mol-1 and 33.58 J K-1 mol-1 for liquid and gas, respectively.
- The molar volume of a certain solid is 161.0 cm3 mol−1 at 1.00 atm and 350.75 K, its melting temperature. The molar volume of the liquid at this temperature and pressure is 163.3 cm3 mol−1. At 100 atm the melting temperature changes to 351.26 K. Calculate the enthalpy and entropy of fusion of the solid. E4B.5(b) The molar volume of a certain solid is 142.0 cm3 mol−1 at 1.00 atm and 427.15 K, its melting temperature. The molar volume of the liquid at this temperature and pressure is 152.6 cm3 mol−1. At 1.2 MPa the melting temperature changes to 429.26 K. Calculate the enthalpy and entropy of fusion of the solid.Calculate the change in entropy of the system when 15.0 g of ice at −12.0 °C is converted to water vapour at 105.0 °C at a constant pressure of 1 bar.Calculate the change in molar Gibbs energy of carbon dioxide (treated as a perfect gas) at 20 °c when its pressure is changed isothermally from 1.0 bar to (a) 3.0 bar. (b) 2. 7 x 10-4 atm, its partial pressure in dry air at sea level.