13. Consider the gas-phase equilibrium system represented by the equation: H₂O(g) → H2(g) + O2(g) Given that the forward reaction is endothermic, which of the following changes will decrease the equilibrium amount of H₂O? A. adding more oxygen C. increasing the temperature B. adding a solid phase catalyst D. adding He gas 14. According to the Bronsted-Lowry Theory an acid breaks up into A an acid and a proton C a coniunate base and a proton
13. Consider the gas-phase equilibrium system represented by the equation: H₂O(g) → H2(g) + O2(g) Given that the forward reaction is endothermic, which of the following changes will decrease the equilibrium amount of H₂O? A. adding more oxygen C. increasing the temperature B. adding a solid phase catalyst D. adding He gas 14. According to the Bronsted-Lowry Theory an acid breaks up into A an acid and a proton C a coniunate base and a proton
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 51QAP: . For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular...
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