47.0 g of liquid benzene, C6H6, is isothermally vaporized at 80.1°C, its boiling point, and constant pressure of 1.20 atm. The molar heat of vaporization of benzene is 30.8 kJ/mol. Assume the volume of the liquid is negligible. Include the sign of each answer below. (a) Calculate q, the heat for the process. kJ (b) Calculate w, the work done by the process. KJ (c) Calculate AE for the process. KJ

47.0 g of liquid benzene, C6H6, is isothermally vaporized at 80.1°C, its boiling point, and constant pressure of 1.20 atm. The molar heat of vaporization of benzene is 30.8 kJ/mol. Assume the volume of the liquid is negligible. Include the sign of each answer below. (a) Calculate q, the heat for the process. kJ (b) Calculate w, the work done by the process. KJ (c) Calculate AE for the process. KJ

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate AGᵒrxn in kJ for the following reaction at 550.0 K. CaCO3(s) CaO(s) + CO₂(g) -89040 O 756.8 O 80.99 O 259.4 AH° +170.2 kJ; AS°= +162.2 J/K
Determine the ΔH of formation for sulfur trioxide gas if: 2 SO2 (g) + O2 (g) --> 2 SO3 (g) ΔH = -300 kJ SO2 (g) --> O2 (g) + S (s) ΔH = 200 kJ The standard state of sulfur is S (s). -500 kJ/mol -400 kJ/mol - 350 kJ/mol +200 kJ/mol +100 kJ/mol
Determine the ΔH of formation for sulfur trioxide gas if: 2 SO2 (g) + O2 (g) --> 2 SO3 (g) ΔH = -300 kJ SO2 (g) --> O2 (g) + S (s) ΔH = 200 kJ The standard state of sulfur is S (s). - 350 kJ/mol -500 kJ/mol +200 kJ/mol +100 kJ/mol -400 kJ/mol
Using the values provided in the table below, calculate ΔHr for the following reaction: 2CO2(g) + 4H2O(g) → 2CH3OH(l) + 3O2(g) a. -2158 kJ mol–1 b. 1354 kJ mol–1 c. -402 kJ mol–1 d. -435 kJ mol–1 e. -1354 kJ mol–1
Calculate the ΔS of vaporization (in J/mol∙K) which boils at 728.7 oC. Its heat of vaporization, ΔHov, is 82.8 kJ/mole.
Calculate ΔHf for HCN(g) at 25°C, given the following related reaction at 25°C, 2 NH3(g) + 3 O2(g) + 2 CH4(g) ---> 2 HCN(g) + 6 H2O(g); ΔHrxn = -870.8 kJ and the heats of formation of some species are ΔHf = -80.3 kJ/mol for NH3(g), -74.6 kJ/mol for CH4, and -241.8 kJ/mol for H2O(g). Answers are in kJ/mol.
The value of ΔE for a system that performs 190 kJ of work on its surroundings and gains 250 kJ of heat is in kj?
Given the following thermochemical equations, find ΔH° for the following reaction: 2NH3(g) + 2O2(g) ⟶ N2O(g) + 3H2O(l) ΔH˚ = ? 2NH3(g) + 4SO3(g) ⟶ N2O(g) + 4SO2(g) + 3H2O(l) ΔH˚ = -290 kJ 2SO3(g) ⟶ 2SO2(g) + O2(g) ΔH˚ = 197 kJ
Consider the following reaction: Sr(OH)2(s) → Sr2+(aq) + 2 OH-(aq) ΔHorxn = -19.3 kJ/ mol Sorxn = -218.3 J/ K mol Which of the following statements is true? Group of answer choices: - the reaction is always non-spontaneous - The reaction is nonspontaneous at all temperatures - The reaction is spontaneous only at high temperature - The reaction is spontaneous only at low temperature - ΔG < 0 and the reaction is always spontaneous