   Chapter 15.3, Problem 15.3CYU

Chapter
Section
Textbook Problem

A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reactionC6H10I2 ⇄ C6H10 + I2has come to equilibrium at 35 °C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.

(a)

Interpretation Introduction

Interpretation: Interpretation: The concentration of C6H10I2 and C6H10 at equilibrium has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

The equilibrium constant K=[C]c[D]d[A]a[B]b

Explanation

From the table,

 Equation C6H10I2 C6H10 I2 Initail concentration 0.050 0 0 Change concentration -0.035 +0.035 +0.035 Equilibrium concentration 0.050-1(0.035)=0.015M 1(0.035)=0.035M 0.035

The concentration of C6H10I2 and C6H10 at equilibrium is 0

(b)

Interpretation Introduction

Interpretation: The equilibrium constant for the given reaction has to be identified.

Concept Introduction: At equilibrium the concentration of the reaction and the product is equated to a constant K, where K is known as the equilibrium

If a reaction is as aA+bBcC+dD ,

The equilibrium constant K=[C]c[D]d[A]a[B]b

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