The following thermochemical equation is for the reaction of hydrogen sulfide(g) with water(l) to form hydrogen(g) and sulfur dioxide(g). H2S(g) + 2H2O(g)3H2(g) + SO2(g) H = 207 kJ When 11.2 grams of hydrogen sulfide(g) react with excess water(l), kJ of energy are _________(evolved or absorbed.)
The following thermochemical equation is for the reaction of hydrogen sulfide(g) with water(l) to form hydrogen(g) and sulfur dioxide(g). H2S(g) + 2H2O(g)3H2(g) + SO2(g) H = 207 kJ When 11.2 grams of hydrogen sulfide(g) react with excess water(l), kJ of energy are _________(evolved or absorbed.)
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section4.6: Reaction Enthalpies For Chemical Reactions
Problem 4.9CE
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The following thermochemical equation is for the reaction of hydrogen sulfide(g) with water(l) to form hydrogen(g) and sulfur dioxide(g).
H2S(g)
- +
2H2O(g)3H2(g)
- +
SO2(g)
- H =
207
- kJ
When 11.2 grams of hydrogen sulfide(g) react with excess water(l), kJ of energy are _________(evolved or absorbed.)
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