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QUESTION 9 Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H₂2(1)→ 2 H₂O(l) + O₂(g) AH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pres -0.0217 kJ -2.31 × 104 kJ -23.1 kJ O-11.5 kJ 1.44 kJ

QUESTION 9 Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2 H₂2(1)→ 2 H₂O(l) + O₂(g) AH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pres -0.0217 kJ -2.31 × 104 kJ -23.1 kJ O-11.5 kJ 1.44 kJ

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 31PS: A volume of 1.50 L of argon gas is confined in a cylinder with a movable piston under a constant...
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O 4.62 J/g °C 7.00 J/g°C 2.20 J/g°C 1.79 J/g°C 2.80 J/g °C QUESTION 9 Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reacţion: 2 H₂O₂(1)→ 2 H₂O(l) + O₂(g) AH = -196 kJ 6 any on 296 R to 398 Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure. -0.0217 kJ -2.31 × 104 kJ -23.1 kJ O -11.5 kJ 1.44 kJ QUESTION 10 In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) + 2 O2(g) → CO2(g) + 2 H₂O(0) AH-890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure. 106.kJ
Transcribed Image Text:O 4.62 J/g °C 7.00 J/g°C 2.20 J/g°C 1.79 J/g°C 2.80 J/g °C QUESTION 9 Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reacţion: 2 H₂O₂(1)→ 2 H₂O(l) + O₂(g) AH = -196 kJ 6 any on 296 R to 398 Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure. -0.0217 kJ -2.31 × 104 kJ -23.1 kJ O -11.5 kJ 1.44 kJ QUESTION 10 In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water: CH4(g) + 2 O2(g) → CO2(g) + 2 H₂O(0) AH-890.0 kJ Calculate the value of q (kJ) in this exothermic reaction when 1.90 g of methane is combusted at constant pressure. 106.kJ
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