   Chapter 5.8, Problem 2.2ACP

Chapter
Section
Textbook Problem

For the purposes of this analysis, let us use octane (C8Hl8) as a substitute for the complex mixture of hydrocarbons in gasoline. Data you will need for this question (in addition to the data in Appendix L) are:ΔfH° [C8H18(ℓ)] = −250.1 kJ/molDensity of ethanol = 0.785 g/mLDensity of octane = 0.699 g/mLCompare the energy produced per liter of the two fuels. Which produces more energy for a given volume (something useful to know when filling your gas tank)?

Interpretation Introduction

Interpretation:

Compare the energy produced per liter of the fuels and the fuel which produces more energy has to be identified

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

From the question the two gases are ethanol and octane,

Density of ethanol is 0.785g/mL

Density of octane is 0.699g/mL

Formation constant of octane is -250.1kJ/mol

For ethanol per liter:

q=-26.82kJ/g×785g/L =-2

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