9. [ Calculate AH for the process in which Cl2(g) initially at 298.15 K at 1 bar is heated to 690. K at 1 bar. Use the temperature-dependent heat capacity for Cl₂(g) below. How large is the relative error if the molar heat capacity is assumed to be constant at its value of 298.15 K over the temperature interval? CP,m= 33.95 J K-¹ mol-¹ for Cl2(g) at 298.15 K. Cp.m JK-1mol-1 = 22.85 +0.06543 – 1.2517 x 10-4+1.1484 x 10-7 K

9. [ Calculate AH for the process in which Cl2(g) initially at 298.15 K at 1 bar is heated to 690. K at 1 bar. Use the temperature-dependent heat capacity for Cl₂(g) below. How large is the relative error if the molar heat capacity is assumed to be constant at its value of 298.15 K over the temperature interval? CP,m= 33.95 J K-¹ mol-¹ for Cl2(g) at 298.15 K. Cp.m JK-1mol-1 = 22.85 +0.06543 – 1.2517 x 10-4+1.1484 x 10-7 K

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 66AP

See similar textbooks

Similar questions

If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is CT- = 56.990.1202T J/mol.K, how much heat is needed?
For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
The following are values of heat capacity for nitrogen gas; Temp K Cv J/mol. K 300 20.8 400 20.9 500 21.2 600 21.8 700 22.4 800 23.1 900 23.7 1000 24.3 1100 24.9 Using the general formula Cv = A BT C/T2, find values of A, B, and C that fit the given data.
Use the two appropriate values of R to determine a conversion between L. atm and J.
at if Hess’s law were not true? What are some possible repercussions this would have?
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
Use the heat capacities of the products and reactants of the thermite reaction and the calculated H of the process to estimate the temperature of the reaction. Assume that all of the heat generated goes to increasing the temperature of the system.
A 237-g piece of molybdenum, initially at 100.0 C, is dropped into 244 g of water at 10.0 C. When the system comes to thermal equilibrium, the temperature is 15.3 C. What is the specific heat capacity of molybdenum?
The standard enthalpy of formation of H2O(l) at 298 K is 285.8 kJ/mol. Calculate the change in internal energy for the following process at 298 K and 1 atm: H2O(l)H2(g)+12O2(g)E=? (Hint: Using the ideal gas equation, derive an expression for work in terms of n, R, and T.)
Apistonhaving0.033 mol ofgas at 35.0Cexpands from0.77 Lto 2.00L.Calculate the work performed if theexpansion occurs a against an externalpressure of 0.455atm,andbreversibly.