Chapter 14.4, Problem 14.7CYU

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# Using the rate constant for HI decomposition given in this example, calculate the concentration of HI after 12 minutes if [HI]0 = 0.010 mol/L.

Interpretation Introduction

Interpretation: The concentration of HI after 12 mins has to be calculated.

Concept Introduction:

The rate of reaction is the quantity of formation of product or the quantity of reactant used per unit time.  The rate of reaction doesn’t depend on the sum of amount of reaction mixture used.

The raise in molar concentration of product of a reaction per unit time or decrease in molarity of reactant per unit time is called rate of reaction and is expressed in units of mol/(L.s).

Integrated rate law for second order reactions:

Taking in the example of following reaction,

aAproducts

And the reaction follows second order rate law,

Then the relationship between the concentration of A and time can be mathematically expressed as,

1[A]t=kt+1[A]0

The above expression is called as integrated rate for second order reactions.

Explanation

The concentration of HI after 12Â mins is calculated as,

â€‚Â -Î”[R]Î”tÂ =Â k[R]2,TheÂ relationÂ canÂ beÂ transformedÂ into,1[R]tÂ =Â 1[R]0Â =Â ktGiven:[HI]tÂ =Â ?[HI]0Â =Â 0.010Â mol/LkÂ =Â 30Â Â L/mol.minÂ tÂ =Â 12Â minsTherefore,1[R]tÂ -Â 1[R]0Â =Â kt1[HI]t-Â 1[HI]0Â =Â ktÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 1[HI]t-Â (1

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