(a) Explanation Given The activation energy of the reaction is 75.5 kJ/mol . The initial temperature of the reaction is 20 ° C . The rate constant at 20 ° C is 2.75 × 10 − 2 s − 1 . The final temperature of the reaction is 60 ° C . The conversion of temperature from ° C into Kelvin is done as, T ( K ) = T ( ° C ) + 273 Hence, the conversion of temperature from 20 ° C into Kelvin is, T 1 ( K ) = ( 20 + 273 ) K = 293 K The conversion of temperature from 60 ° C into Kelvin is, T 2 ( K ) = ( 60 + 273 ) K = 333 K The conversion of energy from kJ/mol into J/mol is done as, 1 kJ/mol = 10 3 J/mol Hence, the conversion of energy from 75.5 kJ/mol into J/mol is, 75.5 kJ/mol = 75.5 × 10 3 J/mol = 7.55 × 10 4 J/mol The rate constant of the given reaction at 60 ° C is calculated by the formula, ln ( k 1 k 2 ) = ( E a R ) ( 1 T 2 − 1 T 1 ) Where, k 1 is the initial rate constant of the reaction (b) Interpretation Introduction To determine: The value of rate constant at 60 ° C for the given reaction. (c) Interpretation Introduction To determine: The assumption required to calculate correct answers in part (a) an (b).

14th Edition

ISBN: 9780134554570

Author: Brown

Publisher: PEARSON

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Chapter 14, Problem 61E

(a)

Interpretation Introduction

To determine: The value of rate constant at 60 °C for the given reaction.

(b)

Interpretation Introduction

To determine: The value of rate constant at 60 °C for the given reaction.

(c)

Interpretation Introduction

To determine: The assumption required to calculate correct answers in part (a) an (b).

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Chapter 14, Problem 60E

Chapter 14, Problem 62E

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