(a)
Interpretation:
The molar change in chemical potential of an ideal gas which expands by
Concept introduction:
The chemical potential is the energy absorbed or released in a
(b)
Interpretation:
The molar change in chemical potential of an ideal gas which expands by
Concept introduction:
The chemical potential is the energy absorbed or released in a chemical reaction or in phase transition. Chemical potential shows the change in Gibbs function with the change in composition of mixture.
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Chapter 4 Solutions
Bundle: Physical Chemistry, 2nd + Student Solutions Manual
- Here you are invited to explore the thermodynamic properties of a gas and its ability to condense to a liquid. Suppose that a gas obeys the van der Waals equation of state with the repulsive effects much greater than the attractive effects (that is, neglect the parameter a). (a) Find an expression for the change in molar Gibbs energy when the pressure is changed from pi to pf. (b) Is the change greater or smaller than for a perfect gas? (c) Estimate the percentage difference between the van der Waals and perfect gas calculations for carbon dioxide undergoing a change from 1.0 atm to 10.0 atm. (d) At the critical point of the gas, dp/dV = 0 and d2p/dV2 = 0. These relations identify the point of inflexion of the isotherms as shown. Show that a gas described by the equation of state p = nRT/V - an2/V2 + bn3/V3 shows critical behaviour, and express the critical constants in terms of the parameters a and b.arrow_forward[3] (b) Formulate the criteria of spontaneity at constant volume and pressure by using the Helmholtz energy (A) and Gibbs energy (G)? (CSLO 2,arrow_forwardCalculate (a) the (molar) Gibbs energy of mixing, (b) the(molar) entropy of mixing when the two major componentsof air (nitrogen and oxygen) are mixed to form air at 298 K.The mole fractions of N2 and 0 2 are 0.78 and 0.22. respectively. (c) Is the mixing spontaneous?arrow_forward
- (a) An ideal gas of mass 4.5 g and molar mass of 17 g.mole-1 occupies 12.7 L at 310 K. Answer the following questions based on the conditions presented. (i) Calculate the work done under a constant external pressure of 30 kPa until the volume of gas has increased by 3.3 L. (ii) Calculate the work done in an isothermal and reversible expansion process resulting in a final volume of 16L. (iii) If the gas has a molar heat capacity of 30.8 J.mol-1.K-1 and is subjected to a constant volume process until it reaches a temperature of 350K, calculate the heat transfer in kJ.mol-1 of the gas. (b) Calculate the standard enthalpy of formation of N2O5 (g) from N2 (g) and O2 (g), in kJ. mol-1, from the following data: 2NO(g) + O2(g) ® 2NO2(g) DH = -114.1 kJ 4NO2(g) + O2(g) ® 2N2O5(g) DH = -110.2 kJ N2(g) + O2(g) ® 2NO(g) DH = +180.5 kJarrow_forwardThe standard state of a substance used to be defined as 1 atm at the specified temperature. By how much does the current definition of standard chemical potential (at 1 bar) differ from its former value at 298.15 K?arrow_forwardCalculate (a) the standard reaction entropy and (b) the change in entropyof the surroundings (at 298 K) of the reaction N2(g) + 3 H2(g) → 2 NH3(g). (c) Hence calculate the standard Gibbs energy of the reaction.arrow_forward
- 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.arrow_forward1. 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=?.arrow_forwardAt 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/molarrow_forward
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