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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It is sometimes appropriate to express the temperature dependence of the heat capacity by the empirical expression Cp,m = a + BT+yT² =a+ßT+yT² . Use this expression to estimate the standard enthalpy of combustion of methane at 350 K. Use the standard enthalpy tables in the back of your book in the "Resource Section" (you can also look this up on the internet) and the following data for the empirical constants: 2C.7 a /(J K¹ mol¹) 14.16 26.86 25.72 30.36 B/(mJ K-¹ mol¯¹) 7/(µJ K-¹ mol¯¹) 75.5 -17.99 6.97 -0.82 12.98 -3.868 9.61 1.184 CH4 (g) CO₂ (g) O₂ (g) H₂O (1) Note that for ß: mJ = 10³ J and for y: µJ=106 J
The standard enthalpy of formation of HCe (g) at 298 K is equal to -92.3 kJ mol-4. The constant-pressure molar heat capacity in this temperature range is given by: Cp,m (H2)/J.K-1.mol-1 = 27.28 + 3.25 x 10-3 T+ 0.50 x 105 T-2 Cp,m (Cl2)/J.K-1.mol-1 = 36.90 + 0.25 x 10-3 T - 2.84 x 105 T-2 %3D Cp.m (HCl2)/J.K-1.mol-1 = 26.53 + 4.60 x 10-3 T+ 1.09 x 105 Calculate the enthalpy formation of HCe (g), AH (in kJ.mol¯-), at 1000 K. [Give your final answer to 3 significant figures].
A 1.000-g gaseous mixture of CH4 and C2H6 at 1 bar and 298 K is burned in a bomb calorimeter. The calorimeter contains 1.500 kg of water initially at 25.00oC. After equilibrium is reached by the system, the final temperature is 33.00oC. The heat capacity of the calorimeter is 318.0 J/oC. The specific heat capacity of water is 4.186 J/g-oC. Calculate the % volume analysis of the fuel. Please provide COMPLETE solution. it should have final answer. not only formulas Tnx..
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.
Carbon dioxide gas with a mass of 88 g is isothermally compressed at a fixed external pressure of 15 bar, with a speed of 298 K and a final pressure of 10 bar from 1 bar. Interpret the results by finding the quantities Δu, Δh, w, Q, Δs, Δa, g and Δsaverage, Δssystem in the event.
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 ?
3. Use the appropriate data from the table to calculate the change in enthalpy for this reaction: Mg) + 2HClag) > M9CI2(ag) + H2(9) (aq) Species AH", , kJ/1mol HCl(g) -92.30 HCl(aq) -167.2 MgCl(s) -641.6 MgCla(aq) -796.9 H,O(1) -285.83 4. Using your answer for question #3, how much energy would be produced from the reaction of 0.680g of Mg with excess hydrochloric acid?
Knowing that the molar heat capacity at constant pressure of CO₂ has the form Cp,m = (a + b + c/T²) J mol-¹K-¹, where a= 44.22, b= 8.79 x 10-³ K-¹, and c= -8.62 x 105 K 2,calculate how much heat can absorb 1.5 moles of this gas when the temperature is increased from 25°C to 150°C. NOTE: Give your answer in kJ mol-1

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