Hydrogen peroxide can decompose to water and oxygen by the following reaction:\[ 2 \, \text{H}_2\text{O}_2 (l) \rightarrow 2 \, \text{H}_2\text{O}(l) + \text{O}_2 (g) \quad \Delta H = -196 \, \text{kJ} \]Calculate the value of \( q \) when 5.00 g of \(\text{H}_2\text{O}_2 (l)\) decomposes at constant pressure.*Use the editor to format your answer*

For calculating amount of heat , given equation must be balanced .if balanced then use unitry method

Hydrogen peroxide can decompose to water and oxygen by the following reaction: 2 H2O2 (1) → 2 H20(1) + O2 (g) AH = -196 kJ Calculate the value of q when 5.00 g of H2O2 (1) %3D decomposes at constant pressure. Use the editor to format your answer

Hydrogen peroxide can decompose to water and oxygen by the following reaction: 2 H2O2 (1) → 2 H20(1) + O2 (g) AH = -196 kJ Calculate the value of q when 5.00 g of H2O2 (1) %3D decomposes at constant pressure. Use the editor to format your answer

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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