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Water gas, a mixture of carbon monoxide and hydrogen, is produced by treating carbon (in the form of coke or coal) with steam at high temperatures. (See Study Question 83.) C(s) + H 2 O(g) → CO(g) + H 2 (g) Not all of the carbon available is converted to water gas since some is burned to provide the heat for the endothermic reaction of carbon and water. What mass of carbon must be burned (to CO 2 gas) to provide the energy to convert 1.00 kg of carbon to water gas?

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Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

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Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 5, Problem 90GQ
Textbook Problem
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Water gas, a mixture of carbon monoxide and hydrogen, is produced by treating carbon (in the form of coke or coal) with steam at high temperatures. (See Study Question 83.)

C(s) + H2O(g) → CO(g) + H2(g)

Not all of the carbon available is converted to water gas since some is burned to provide the heat for the endothermic reaction of carbon and water. What mass of carbon must be burned (to CO2 gas) to provide the energy to convert 1.00 kg of carbon to water gas?

Interpretation Introduction

Interpretation:

The energy required to convert 1kg of carbon has to be calculated.

Concept Introduction:

The standard enthalpy of formation is the enthalpy change for the formation of 1mol of the compound directly from its component elements in their standard states.

Enthalpy change for the reaction ΔrH0Chemistry & Chemical Reactivity, Chapter 5, Problem 90GQ ΣnΔfH0(products)-ΣnΔfH0(reactants)

Explanation of Solution

Given,

Mass1Kg

ΔfH0(C)= 0 KJ/mol 

ΔfH0(H2O)-241.8kJ/mol

ΔfH0(CO)-110.54kJ/mol

ΔfH0(H2)0J/mol

Using Hess law,

  ΔrH0ΣnΔfH0(products)-ΣnΔfH0(reactants)

  ΔrH° =(-110

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Chemistry & Chemical Reactivity
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