Explanation Given Mass of hydrogen peroxide ( H 2 O 2 ) is 5.00 g . Pressure is kept constant. The amount of heat released by the decomposition of the given moles of H 2 O 2 ( Δ H ) is − 196 kJ . The given decomposition reaction is, 2H 2 O 2 ( l ) → 2H 2 O ( l ) + O 2 ( g ) The molar mass of H 2 O 2 = 2 H + 2 O = ( ( 2 × 1 ) + ( 2 × 16 ) ) g / mol = 34 g / mol Formula The number of moles of a substance is calculated using the formula, Number of moles = Given mass Molar mass of

Laboratory Experiments for Chemistry: The Central Science (13th Edition)

13th Edition

ISBN: 9780321949912

Author: Theodore E. Brown, John H. Nelson, Kenneth C. Kemp

Publisher: PEARSON

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Chapter 13, Problem 79E

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To determine: The quantity of heat released when 5.00 g of hydrogen peroxide (H2O2) decomposes at a constant pressure.

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Chapter 13, Problem 78E

Chapter 13, Problem 80E

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Chapter 13 Solutions

Laboratory Experiments for Chemistry: The Central Science (13th Edition)

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Ch. 13.4 - 4.17 Specify what ions are present in solution...Ch. 13.4 - Prob. 13.6.2PE Ch. 13.5 - Prob. 13.7.1PE Ch. 13.5 - Acetone. CH3COCH3, is a nonelectrolyte;...Ch. 13.5 - 4.21 Using solubility guidelines, predict whether...Ch. 13.5 - Prob. 13.8.2PE Ch. 13.5 - Prob. 13.9.1PE Ch. 13.5 - Prob. 13.9.2PE Ch. 13.5 - 4 3 Use the molecular representations shown here...Ch. 13.5 - The concept of chemical equilibrium is very...Ch. 13.5 - 4 5 You are presented with a white solid and told...Ch. 13.5 - Which of the following ions will always be a...Ch. 13 - Which element is oxidized, and which is reduced in...Ch. 13 - Which of the following are redox reactions? 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The quantity of heat released when 5.00 g of hydrogen peroxide ( H 2 O 2 ) decomposes at a constant pressure.

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To determine: The quantity of heat released when 5.00 g of hydrogen peroxide (H2O2) decomposes at a constant pressure.

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Chapter 13 Solutions