When determining the energy of a reaction where 0.250 mol of a substance with a ΔHcomb = -2250.0 kJ/mol reacts, we perform the attached calculation. Why can’t we simply say that the energy of the reaction is -2250.0 kJ? Is it because it is J, or kj/mol. I thought that -2250.0 kJ is the enthalpy of that particular scenario. Molar enthalpy requires we divide the by the number of moles so that we have a volume PER MOLE rather than per 0.250 mol. I don't really understand.
When determining the energy of a reaction where 0.250 mol of a substance with a ΔHcomb = -2250.0 kJ/mol reacts, we perform the attached calculation. Why can’t we simply say that the energy of the reaction is -2250.0 kJ? Is it because it is J, or kj/mol. I thought that -2250.0 kJ is the enthalpy of that particular scenario. Molar enthalpy requires we divide the by the number of moles so that we have a volume PER MOLE rather than per 0.250 mol. I don't really understand.
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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1. When determining the energy of a reaction where 0.250 mol of a substance with a ΔHcomb = -2250.0 kJ/mol reacts, we perform the attached calculation. Why can’t we simply say that the energy of the reaction is -2250.0 kJ?
Is it because it is J, or kj/mol. I thought that -2250.0 kJ is the enthalpy of that particular scenario. Molar enthalpy requires we divide the by the number of moles so that we have a volume PER MOLE rather than per 0.250 mol. I don't really understand.
Transcribed Image Text:-2250.0 kJ
x kJ
-2250.0 kJ
OR 0.250 mol
1mol
0.250 mol
1mol
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