Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Calculate the difference, AH-AE=A(PV) for the combustion reaction of 1 mole of methane. (Assume standard state conditions and 298 K for all reactants and products.) -1094kJ

Calculate the difference, AH-AE=A(PV) for the combustion reaction of 1 mole of methane. (Assume standard state conditions and 298 K for all reactants and products.) -1094kJ

Chemistry
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
icon
Related questions
Question
100%
Combustion of methane. Refer to the second question in the attached image. Apparently with one mole of methane combustion the pressure and volume are different for gasses in the reaction.
Course Contents » .. » Homework set #5 > Enthalpy of Combustion -- Alkanes Write a balanced equation for the combustion of CH (g) (methane) i.e. its reaction with O,(g) forming the products CO2(g) and H20(). Given the following standard heats of formation: AH of CO2(g) is -393.5 kJ/mol AH of H20(1) is -286 ki/mol AH of CH,(g) is -74.8 kJ/mol What is the standard heat of reaction (AH) for the combustion reaction of CH(g)? -890.7 kJ You are correct. Previous Tries Your receipt no. is 164-687 Calculate the difference, AH-AE=A(PV) for the combustion reaction of 1 mole of methane. (Assume standard state conditions and 298 K for all reactants and products.) -1094KJ The ideal gas law must be used. The incremental change in volume due to liquids is neglected (cf the volume of 1 mole of H,0 Be careful to account for the total change in number of moles of gas molecules (be sure the s Note that certain alkanes are gases in the standard state.
Transcribed Image Text:Course Contents » .. » Homework set #5 > Enthalpy of Combustion -- Alkanes Write a balanced equation for the combustion of CH (g) (methane) i.e. its reaction with O,(g) forming the products CO2(g) and H20(). Given the following standard heats of formation: AH of CO2(g) is -393.5 kJ/mol AH of H20(1) is -286 ki/mol AH of CH,(g) is -74.8 kJ/mol What is the standard heat of reaction (AH) for the combustion reaction of CH(g)? -890.7 kJ You are correct. Previous Tries Your receipt no. is 164-687 Calculate the difference, AH-AE=A(PV) for the combustion reaction of 1 mole of methane. (Assume standard state conditions and 298 K for all reactants and products.) -1094KJ The ideal gas law must be used. The incremental change in volume due to liquids is neglected (cf the volume of 1 mole of H,0 Be careful to account for the total change in number of moles of gas molecules (be sure the s Note that certain alkanes are gases in the standard state.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Thermodynamics
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS