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: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 5.62QE: A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup...
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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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