Hydrogen peroxide (H2O2) decomposes to water and oxygen at constant pressure by the following balanced reaction equation reaction: 2 H2O2(1) → 2 H20(1) + O2(g) AH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.50 g of hydrogen peroxide decomposes at constant pressure. -13.0 kJ -6.50 kJ -43.6 kJ -88.2 kJ -21.4 kJ
Hydrogen peroxide (H2O2) decomposes to water and oxygen at constant pressure by the following balanced reaction equation reaction: 2 H2O2(1) → 2 H20(1) + O2(g) AH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.50 g of hydrogen peroxide decomposes at constant pressure. -13.0 kJ -6.50 kJ -43.6 kJ -88.2 kJ -21.4 kJ
Chemistry by OpenStax (2015-05-04)
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ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter16: Thermodynamics
Section: Chapter Questions
Problem 56E: Nitric acid, HNO3, can be prepared by the following sequence of reactions:...
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![Hydrogen peroxide (H2O2) decomposes to water and oxygen at constant
pressure by the following balanced reaction equation reaction:
2 H2O2(1) → 2 H20(1) + O2(g) AH = -196 kJ
Calculate the value of q (kJ) in this exothermic reaction when 4.50 g of
hydrogen peroxide decomposes at constant pressure.
-13.0 kJ
-6.50 kJ
-43.6 kJ
-88.2 kJ
-21.4 kJ](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3571432d-4c13-4269-b396-3277937efc65%2F724a51aa-f499-4c0f-b168-1ba680469565%2Fd9i6d6.jpeg&w=3840&q=75)
Transcribed Image Text:Hydrogen peroxide (H2O2) decomposes to water and oxygen at constant
pressure by the following balanced reaction equation reaction:
2 H2O2(1) → 2 H20(1) + O2(g) AH = -196 kJ
Calculate the value of q (kJ) in this exothermic reaction when 4.50 g of
hydrogen peroxide decomposes at constant pressure.
-13.0 kJ
-6.50 kJ
-43.6 kJ
-88.2 kJ
-21.4 kJ
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