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

Chemistry: The Central Science (14th Edition)

14th Edition

ISBN: 9780134414232

Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus

Publisher: PEARSON

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Chapter 5.4, Problem 5.4.2PE

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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 5.4, Problem 5.4.1PE

Chapter 5.5, Problem 5.5.1PE

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Chemistry: The Central Science (14th Edition)

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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 5 Solutions