   # The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to HI. The rate defined below is constant at 1.20 × 10 −4 mol/L · s. 2HI ( g ) → Au H 2 ( g ) + I 2 ( g ) Rate = − Δ [ HI ] Δ t = k = 1.20 × 10 − 4 mol/L ⋅ s a. If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction. b. How long will it take for all of the 0.250 M HI to decompose? ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 11, Problem 48E
Textbook Problem
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## The decomposition of hydrogen iodide on finely divided gold at 150°C is zero order with respect to HI. The rate defined below is constant at 1.20 × 10−4 mol/L · s. 2HI ( g ) → Au H 2 ( g ) + I 2 ( g ) Rate   =   − Δ [ HI ] Δ t   =   k =   1.20   ×     10 − 4 mol/L   ⋅   s a. If the initial HI concentration was 0.250 mol/L, calculate the concentration of HI at 25 minutes after the start of the reaction.b. How long will it take for all of the 0.250 M HI to decompose?

(a)

Interpretation Introduction

Interpretation: The rate constant for the zero order reaction with respect to HI for the decomposition of hydrogen iodide on finely divided gold is given. By using this value, the concentration of HI at given time and the time for the decomposition of given concentration of HI is to be calculated.

Concept introduction: The change observed in the concentration of a reactant or a product per unit time is known as the rate of the particular reaction. The differential rate law provides the rate of a reaction at specific reaction concentrations.

To determine: The concentration of HI at 25minutes after the start of reaction.

### Explanation of Solution

Given

The initial concentration of HI is 0.250mol/L .

The rate constant is 1.20×104mol/Ls .

The time elapsed is 25minutes .

The zero order reaction of decomposition of hydrogen iodide on finely divided gold is, 2HI(g)H2(g)+I2(g)

It is assumed that the concentration of HI after time t is x .

The conversion of minute into second (s) is done as,

1minute=60s

Hence, the conversion of 25minutes into second is,

25minutes=(25×60)s=1500s

Formula

The formula of rate of reaction is,

k=Δ[HI]Δt=([H]t[H]0t)

Where,

• k is rate constant

(b)

Interpretation Introduction

Interpretation: The rate constant for the zero order reaction with respect to HI for the decomposition of hydrogen iodide on finely divided gold is given. By using this value, the concentration of HI at given time and the time for the decomposition of given concentration of HI is to be calculated.

Concept introduction: The change observed in the concentration of a reactant or a product per unit time is known as the rate of the particular reaction. The differential rate law provides the rate of a reaction at specific reaction concentrations.

To determine: The time taken to decompose 0.250mol/L HI .

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