5. Use the data in the following tables and answer the following questions. a) The experimental data (table 1.) is from the combustion of ethanol in a bomb calorimeter. Use the data to determine the enthalpy of combustion per mole of ethanol. The quantity of energy transferred to the calorimeter can be solved using the equation Qbomb = Chomb* AT b)Use the standard enthalpies of formation (Table 2) to determine the enthalpy of combustion per mole of ethanol. c) Explain any discrepancies (2 reasons) between the values calculated in questions a. and b. Table 1 Data from Combustion of Ethanol in a Bomb Calorimeter Mass of ethanol 3.26 g Heat capacity of calorimeter 11.7 kJ/°C Initial temperature of calorimeter 21.5°C Final temperature of calorimeter 29.4 °C Table 2 Standard Enthalpies of Formation Substance H₂O( CO₂(g) C₂H₂OH() AH, (kJ/mol) -285.8 -393.5 -235.2

5. Use the data in the following tables and answer the following questions. a) The experimental data (table 1.) is from the combustion of ethanol in a bomb calorimeter. Use the data to determine the enthalpy of combustion per mole of ethanol. The quantity of energy transferred to the calorimeter can be solved using the equation Qbomb = Chomb* AT b)Use the standard enthalpies of formation (Table 2) to determine the enthalpy of combustion per mole of ethanol. c) Explain any discrepancies (2 reasons) between the values calculated in questions a. and b. Table 1 Data from Combustion of Ethanol in a Bomb Calorimeter Mass of ethanol 3.26 g Heat capacity of calorimeter 11.7 kJ/°C Initial temperature of calorimeter 21.5°C Final temperature of calorimeter 29.4 °C Table 2 Standard Enthalpies of Formation Substance H₂O( CO₂(g) C₂H₂OH() AH, (kJ/mol) -285.8 -393.5 -235.2

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

Propane is a gas commonly used to fuel gas grills and camping stoves. The structure of propane is shown below. Write the balanced chemical equation for the combustion of propane. Draw out lewis dot structures to represent all molecules of all products and reactants in this reaction. The number of each molecule should be reflected in the balanced equation. Calculate the heat of combustion for propane using the bond enthalpies in the table. 1.00 mol of propane is used to roast marshmallows. It was determined that the amount of energy absorbed by the marshmallows was only 800 kJ. Explain this observation.
Calculate the enthalpy change for the reaction of magnesium and water using Hess’s Law.
3. Write a balanced chemical reaction for the synthesis of methane (CH4) and liquid water from hydrogen and acetic acid (CH3COOH) and calculate the standard enthalpy of the reaction by using the appropriate enthalpies of formation on page 308 or Appendix 4 in the textbook.
Please help me answer the questions from a to f using the data provided
Show work to support your answer to this question. a) In a study of gaseous xenon, a chemist finds that 27.6 J of energy must be added to increase the temperature of 10.7 g of xenon from 22.7° C to 39.9° C. What is the experimental specific heat value for xenon gas? b) Using the specific heat you calculated for gaseous xenon, how much heat will be required to heat the 10.7 g sample of xenon from 39.9° C to 278.9° C?
Write the balanced chemical equation and draw an enthalpy diagram for the formation of 1 molof sodium chloride from its elements (heat is released).
23
The enthalpy change for a chemical reaction is the sum of the energy consumed in breaking bonds and the energy released during bond formation. One way to determine the overall energy change for a chemical reaction is to apply Hess’s law to add together a group of reactions which can be arranged such that the chemical equations, when combined, give the overall equation we are trying to characterize. a. Write a balanced chemical equation for the combustion of gaseous propane in gaseous oxygen to produce gaseous carbon dioxide and liquid water. C3H8(g)+ O2(g) ---->CO2(g)+ H2O(g) b. Combine the following equations to determine the enthalpy change for the combustion of 1 mole of propane. Assume that solid carbon is graphite. 3C(s,graphite)+4H2(g)--->C3H8(g) ΔHo = -103.8 kJ/mol C(s,graphite)+O2(g)--->CO2(g) ΔHo= -393.5 kJ/mol H2(g)+1/2 O2(g)--->H2O(g) ΔHo= -285.8 kJ/mol kJ/mol…