   Chapter 20, Problem 25PS

Chapter
Section
Textbook Problem

Confirm the statement in the text that oxidation of 1.0 L of methanol to form CO2(g) and H2O(ℓ) in a fuel cell will provide at least 5.0 kW-h of energy. (The density of liquid methanol is 0.787 g/mL. See Study Question 24 for definition of kW-h.)

Interpretation Introduction

Interpretation:

It should be confirmed that oxidation of 1.0L methanol to form CO2(g) and H2O(l) in a fuel cell will provide at least 5.0kWh of energy.

Concept introduction:

• Standard enthalpy of reaction ΔrH0 is the enthalpy change that occurs in a system when matter is transformed by a given chemical reaction, when all reactants and products are in their standard states.
• Enthalpy of formation is the heat released or absorbed in a chemical reaction at constant temperature when simple substances combine into a more complex substance.
• 1kWh=3600kJ
Explanation

Given,

The oxidation reaction of 1.0L methanol to form CO2(g) and H2O(l) can be written as,

CH3OH(l)+1.5O2(g)CO2(g)+2H2O(l)

The standard enthalpy for the above reaction ΔrH0 is, -726.8kJ/mol

Energy from 1.0L of fuel is -17

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