Interpretation: The normal boiling point and the normal standard point are to be calculated for liquid benzene. Whether the obtained result agrees with the value in the mentioned table or not should be explained.
Concept introduction: Normal boiling point is the point when the pressure becomes equal to
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Thermodynamics, Statistical Thermodynamics, & Kinetics
- The expression ΔG / J = enerj85.40 + 36.5 (T / K) of the change in Gibbs energy is found to fit a certain constant pressure process. Calculate the value of ΔS for the process.arrow_forwardWithout carrying out an explicit calculation, explain there lative values of the standard molar entropies (at 298 K) of the following substances: (a) Ne(g) (146 J K-1 mol-1) compared with Xe(g) (170 J K-1 mol-1), (b) H2O(g) (189 J K-1 mol-1) compared with D2O(g) (198 J K-1 mol-1), (c) C(diamond) (2.4 J K-1 mol-1) compared with C(g raphite) (5.7 J K-1 mol-1).arrow_forwardEstimate the enthalpy of vaporization of water at 92.5 °C from its value at 25 °C (44.01 kJ mol−1), given the constant-pressure heat capacities of 75.29 J K−1mol−1 and 33.58 J K−1 mol− 1 for liquid and gas, respectively. ______ kJ/mol. 4 sig. numberarrow_forward
- Estimate 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.arrow_forwardCalculate the entropy and enthalpy of vaporization for 1 mole of water at room temperature (25oC) and 1 atm from these thermodynamic data:Cm,p(H2O, liquid) = 75.29 J/K·mol, Cm,p(H2O, gas) = 33.58 J/K·mol and ∆vapH(H2O) = 40700 J/ mol (at 100oC)arrow_forwardThe change in the Gibbs energy of a certain constant-pressure process is found to fit the expression ΔG/J = −73.1 + 42.8(T/K). Calculate the value of ΔS for the process.arrow_forward
- For a certain constant-pressure process, the change in Gibbs energy was found to fit the expression: G/J = -20+ 10(T/K). What are H and S for the process?arrow_forwardThe molar heat capacity of N2(g) in the range 200 K to 400 K is given by Cp,m/(J K−1 mol−1) = 28.58 + 3.77 × 10–3(T/K). Given that the standard molar entropy of N2(g) at 298 K is 191.6 J K−1 mol−1, calculate the value at 373 K. Repeat the calculation but this time assuming that Cp,m is independent of temperature and takes the value 29.13 J K−1 mol−1. Comment on the difference between the results of the two calculations.arrow_forwardCalculate the change of entropy in the system: Delta S of the surrounding=251 kJ/mol, Gibbs free energy =-54 kJ/mol T=298Karrow_forward
- The differential for the Gibbs function, G, at constant composition is: dG = −S?T + Vdp write the total differential of G, i.e., dG, in terms of partial differentials.arrow_forwardAt 100°C, the standard molar is the enthalpy of vaporization ∆vapH⊖m of water 40.7 kJ mol-1 while the standard molar entropy of vaporization ∆vapS⊖m = 109.1 J mol-1 K-1. The molar standard heat capacities of water as a liquid and water as a gas are, respectively, 75,291J mol-1 K-1 and 33.58 J mol-1 K-1. 6) Calculate both the standard molar enthalpy of vaporization and the standard molar entropy of vaporization at 25°C. It must be assumed that the heat capacities are independent of the temperature.arrow_forwardThe standard Gibbs energy of formation of rhombic sulfur is zero, and that of monoclinic sulfur is +0.33 kJ mol−1 at 25 °C. The standard molar entropy of rhombic sulfur is 31.80 J K−1 mol−1, and that of monoclinic sulfur is 32.6 J K−1 mol−1. At what temperature will the transition occur at 1 bar? _______ K. 3 sig. fig.arrow_forward
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,