Calculate the change in enthalpy AH and entropy AS of 1 kg benzene when heatedfrom 20°C to 80°C and additionally evaporated completely.Take the density of liquid benzene, the heat capacity and the enthalpy of evaporationof benzene as p = 874 g L-1, Cp,m = 82 J mol¹ K and AHvap = 34 kJ mol¹ respectively.

To calculate the change in enthalpy (Δ𝐻) and entropy (Δ𝑆) of 1 kg of benzene when it is heated…

Answered: Calculate the change in enthalpy AH and…

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...

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P3B.4 The molar heat capacity of N,(g) in the range 200 K to 400 K is given by Cm/(JK mol) = 28.58 + 3.77 x 10°(T/K). Given that the standard molar entropy of N,(g) at 298 K is 191.6 J Kmol, calculate the value at 373 K. Repeat the calculation but this time assuming that C, is independent of %3D D.m temperature and takes the value 29.13 J K mol. Comment on the difference between the results of the two calculations.
what is the change in entropy when150 ml of cold (278 k) water is added to 150 ml of nearly boiling(368 k)water? ignore any potential heat loss to the surroundings; only consider the water. assume that for water, ρ=1.00 g⁄ml, c ̅_p=75.3 jk^(-1) mol^(-1), and that each is constant over the given temperature range.
1. (a) In reaching equilibrium, how much heat transfer occurs from 1.2 kg of water at 40°C when it is placed in contact with 1.2 kg of 20°C water? Specific heat of water c=4186 J/(kg°C) Hint: If the masses of water are equal, what is the equilirium temperature of the water mixture? Q= ✓ J (b) What is the change in entropy due to this heat transfer? AS total ✔J/K (c) How much work is made unavailable, taking the lowest temperature to be 20°C? = W unavailable ✓ J
Gaseous SO2Cl2 reacts with liquid water to form hydrogen chloride gas and liquid sulfuric acid. Using data tabulated in Appendix G of your text, calculate the enthalpy change, in units of kJ/mol, for the formation of 2 mol of liquid sulfuric acid.
Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units. Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K. Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.
4. Calculate the work done under isothermal conditions for 5.5 mols of an ideal gas expanding from 10.0 bar to 2.00 bar at –20.0°C both for a reversible (a) and irreversible (b) process. For the latter, Pext = 2.00 bar. The general expression for work is, w=-[P_dV
Calculate the change in entropy that occurs in the system when 1.61 mol of diethyl ether (C4H10O) condenses from a gas to a liquid at its normal boiling point (34.6 °C). The heat of vaporization is 26.5 kJ/mol. Express your answer with the appropriate units. AS = μÅ Value Units ?
Assuming ideal gas behavior, calculate ΔH Assuming ideal gas behavior, calculate q Assuming ideal gas behavior, calculate ΔU w =−2.48×104 J
At 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.

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