The standard enthalpies of formation, at 25.00 °C, of methane (CH4(g)), water (H,O(1)), and carbon dioxide (CO-(g)) are respectively -74.6 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the heat released (in kJ) during the combustion of 17.70 L of methane under a constant pressure of 1.000 atm at 25.00 °C (N.B. combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).
The standard enthalpies of formation, at 25.00 °C, of methane (CH4(g)), water (H,O(1)), and carbon dioxide (CO-(g)) are respectively -74.6 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the heat released (in kJ) during the combustion of 17.70 L of methane under a constant pressure of 1.000 atm at 25.00 °C (N.B. combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Question 2: The standard enthalpies of formation, at 25.00 °C, of methane (CH4(g)), water (H,O(1)), and carbon dioxide (CO-(g)) are respectively -74.6 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the heat released (in kJ) during the combustion of 17.70 L of methane under a constant pressure of 1.000 atm at 25.00 °C (N.B. combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).
Expert Solution
Step 1
To calculate the heat released, first we would calculate the enthalpy change of reaction by writing the balanced chemical reaction of combustion of methane and using the standard enthalpy of formation.
Then we need to calculate the models of methane combusted using the given volume , pressure and temperature.
Using the enthalpy change of reaction and moles we can calculate the heat released.
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