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 favoursN₂0₂(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 occurfaster than the reverse reaction.iii. The forward and reverse reactions are both continuing to occur, but at an equal rate so the netconcentrations 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 beoccurring faster than the forward reaction.

we have given a figure representing an equilibrium mixture of compounds related by the reaction-2NO…

Answered: (a) According to the figure, this…

(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?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

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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