NaOH(s) trial (A) NHẠNO3 (s) trial (B)Part 2: Enthalpy of dissolutiona. Mass of substance dissolved (g)b. Mass of calorimeter (g)c. Mass of calorimeter + water (g)d. Mass of water (g)0.83140.79852.1142.17911.971712.0731e. Total mass of reactants (g)f. Initial temperature of water (°C)g. Final temperature of solution (°C)h. Change in the temperature, AT (°C)i. Moles of solid dissolved in water (mols)j. Heat lost or gained by the water, Aqm (J)k. Heat absorbed by the calorimeter, Aq. (J)I. Heat absorbed or released by the dissolving soluteAq: = Aqm+ Aqc (J)m. Enthalpy of solution, AHrxn (kJ/mol)n. Theoretical enthalpy, calculated AHrxn (kJ/mol)18.018.230.013.6o. Percent error

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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 75AP

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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.
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?
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