   # The standard enthalpy of combustion of ethene gas, C 2 H 4 (g), is −1411.1 kJ/mol at 298 K. Given the following enthalpies of formation, calculate Δ H f ° for C 2 H 4 (g). CO 2 ( g ) − 393.5 KJ/mol H 2 O ( l ) − 285.8 KJ/mol ### 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 7, Problem 84E
Textbook Problem
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## The standard enthalpy of combustion of ethene gas, C2H4(g), is −1411.1 kJ/mol at 298 K. Given the following enthalpies of formation, calculate Δ H f ° for C2H4(g). CO 2 ( g ) − 393.5   KJ/mol H 2 O ( l ) − 285.8   KJ/mol

Interpretation Introduction

Interpretation: Standard enthalpy of formation of ethane gas (C2H4) has to be calculated.

Concept introduction

Standard Enthalpy of formation ( ΔHf0 ): The standard enthalpy of formation is defined as the change in enthalpy when one mole of a substance in the standard state.

Standard condition: 250C and 1 atmosphere pressure.

### Explanation of Solution

Explanation

Standard enthalpy of combustion of ethane gas (C2H4(g)) is -1411.1 kJ/mol at 298K

Given: Standard enthalpy value for given substance in the reaction are,

 Substance and state         ΔHf0 kJ / mol H2O(l)                                  -285.8 CO2(g)                                  -393.5

To calculate standard enthalpy of formation of ethene gas.

Substitute standard enthalpy values into enthalpy change equation.

ΔHo = H0product-H reactant0

-1411.1kJ    = [(-393

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