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(a) According to the figure, this equilibrium favours (b) What may be inferred about the numerical value of K? (c) Which one of the following expressions is true of this equilibrium?

(a) According to the figure, this equilibrium favours (b) What may be inferred about the numerical value of K? (c) Which one of the following expressions is true of this equilibrium?

Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.81P
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The figure represents an equilibrium mixture of compounds related by the reaction: 2 NO(g) = N₂(g) + O₂(g) ∞ Key: (a) According to the figure, this equilibrium favours N₂ 0₂ (b) What may be inferred about the numerical value of K? NO (c) Which one of the following expressions is true of this equilibrium? > i. When enough time has elapsed, all the reactant will be consumed. ii. The greater concentrations of reactant than product is causing the forward reaction to occur faster than the reverse reaction. iii. The forward and reverse reactions are both continuing to occur, but at an equal rate so the net concentrations do not change. iv. The forward and reverse reactions have now entirely ceased. v. Since reactant is found in greater concentration than product, the reverse reaction must be occurring faster than the forward reaction.
Transcribed Image Text:The figure represents an equilibrium mixture of compounds related by the reaction: 2 NO(g) = N₂(g) + O₂(g) ∞ Key: (a) According to the figure, this equilibrium favours N₂ 0₂ (b) What may be inferred about the numerical value of K? NO (c) Which one of the following expressions is true of this equilibrium? > i. When enough time has elapsed, all the reactant will be consumed. ii. The greater concentrations of reactant than product is causing the forward reaction to occur faster than the reverse reaction. iii. The forward and reverse reactions are both continuing to occur, but at an equal rate so the net concentrations do not change. iv. The forward and reverse reactions have now entirely ceased. v. Since reactant is found in greater concentration than product, the reverse reaction must be occurring faster than the forward reaction.
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