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

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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