Chapter 5.8, Problem 2.3ACP

### 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

# What mass of CO2, a greenhouse gas, is produced per liter of fuel (assuming complete combustion)?

Interpretation Introduction

Interpretation:

The mass of CO2 produced per liter of fuel has to be determined.

Concept Introduction:

Heat energy required to raise the temperature of 1g of substance by 1k.Energy gained or lost can be calculated using the below equation.

q=C×m×ΔT

Where,

q= energy gained or lost for a given mass of substance (m),

C =specific heat capacity

ΔT= change in temperature

Explanation

Given,

Molar mass of ethanol is 46.07â€‰g

Molar mass of carbon dioxide is 44.01â€‰g

Molar mass of octane is 114.2â€‰g

Mass of CO2 per liter of ethanol=

=1.000L(785gâ€‰C2H5OH/L)(1molâ€‰C2H5OH46.07gC2H5OH)(2molâ€‰CO21molâ€‰C2H5OH)(44.01gâ€‰CO21molâ€‰CO2â€‰)

=1

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