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of gaseous azomethane (C2H6N2) was added to a flask kept at 400 °C and was allowed 2.00 g to decompose according to the following equation: C2H,N2(g) → N2(g) + C2H6(g) The rate constant for this decomposition is 40.0 min 1 at 400 °C. 2.1. Calculate the half-life (in seconds) for this reaction. 2.2. Calculate the mass (in g) of ethane gas that will be formed in this flask after 2.00 seconds.

of gaseous azomethane (C2H6N2) was added to a flask kept at 400 °C and was allowed 2.00 g to decompose according to the following equation: C2H,N2(g) → N2(g) + C2H6(g) The rate constant for this decomposition is 40.0 min 1 at 400 °C. 2.1. Calculate the half-life (in seconds) for this reaction. 2.2. Calculate the mass (in g) of ethane gas that will be formed in this flask after 2.00 seconds.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Question 2 2.00 g of gaseous azomethane (C2H6N2) was added to a flask kept at 400 °C and was allowed to decompose according to the following equation: C2H,N2(g) → N2(g) + C2H6(g) The rate constant for this decomposition is 40.0 min-1 at 400 °C. 2.1. Calculate the half-life (in seconds) for this reaction. 2.2. Calculate the mass (in g) of ethane gas that will be formed in this flask after 2.00 seconds.
Transcribed Image Text:Question 2 2.00 g of gaseous azomethane (C2H6N2) was added to a flask kept at 400 °C and was allowed to decompose according to the following equation: C2H,N2(g) → N2(g) + C2H6(g) The rate constant for this decomposition is 40.0 min-1 at 400 °C. 2.1. Calculate the half-life (in seconds) for this reaction. 2.2. Calculate the mass (in g) of ethane gas that will be formed in this flask after 2.00 seconds.
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