Direct methanol fuel cells (DMFCs) have shown some promise as a viable option for providing “green” energy to small electrical devices. Calculate for the reaction that takes place in DMFCs: CH 3 OH ( l ) + 3 / 2 O 2 ( g ) → CO 2 ( g ) + 2 H 2 O ( l ) Use values of Δ G f ∘ from Appendix 4.

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Interpretation Introduction Interpretation: The standard cell potential ( E ο ) for the given reaction that takes place in direct methanol fuel cell (DMFCs) is to be calculated. Concept introduction: The standard cell potential is defined as the electromotive force (emf) of a cell when a metal ion electrode is coupled with a hydrogen electrode under standard conditions and hence, is known as standard electrode potential. To determine: The standard cell potential ( E ο ) for the given reaction takes place in direct methanol fuel cell (DMFCs). Explanation The standard free energy of formation is shown below. The given equation is, CH 3 OH ( l ) + 3 2 O 2 ( g ) → CO 2 ( g ) + 2 H 2 O ( l ) . Refer Appendix 4. The standard free energy of formation for the above reaction is, Substance Δ G f ο ( KJ/mol ) CO 2 ( g ) − 394 H 2 O ( l ) − 237 CH 3 OH ( l ) − 166 O 2 ( g ) 0 The standard free energy of reaction is calculated by using the expression below by substituting the standard values of formation, Δ G ο = ∑ n p Δ G f ( products ) ο − ∑ n r Δ G f ( reactants ) ο = Δ G f ( CO 2 ( g ) ) ο + 2 Δ G f ( H 2 O ( l ) ) ο − Δ G f ( CH 3 OH ( l ) ) ο − ( 3 2 ) Δ G f ( O 2 ( g ) ) ο Substitute the required values in the above expression. Δ G ο = ∑ n p Δ G f ( products ) ο − ∑ n r Δ G f ( reactants ) ο = Δ G f ( CO 2 ( g ) ) ο + 2 Δ G f ( H 2 O ( l ) ) ο − Δ G f ( CH 3 OH ( l ) ) ο − ( 3 2 ) Δ G f ( O 2 (

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Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

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Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

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Interpretation Introduction

Interpretation:

The standard cell potential (Eο) for the given reaction that takes place in direct methanol fuel cell (DMFCs) is to be calculated.

Concept introduction:

The standard cell potential is defined as the electromotive force (emf) of a cell when a metal ion electrode is coupled with a hydrogen electrode under standard conditions and hence, is known as standard electrode potential.

To determine: The standard cell potential (Eο) for the given reaction takes place in direct methanol fuel cell (DMFCs).

Explanation of Solution

The standard free energy of formation is shown below.

The given equation is,

CH3OH(l)+32O2(g)→CO2(g)+2H2O(l) .

Refer Appendix 4.

The standard free energy of formation for the above reaction is,

SubstanceΔGfο(KJ/mol)CO2(g)−394H2O(l)−237CH3OH(l)−166O2(g)0

The standard free energy of reaction is calculated by using the expression below by substituting the standard values of formation,

ΔGο=∑npΔGf(products)ο−∑nrΔGf(reactants)ο=ΔGf(CO2(g))ο+2ΔGf(H2O(l))ο−ΔGf(CH3OH(l))ο−(32)ΔGf(O2(g))ο

Substitute the required values in the above expression.

ΔGο=∑npΔGf(products)ο−∑nrΔGf(reactants)ο=ΔGf(CO2(g))ο+2ΔGf(H2O(l))ο−ΔGf(CH3OH(l))ο−(32)ΔGf(O2(

Direct methanol fuel cells (DMFCs) have shown some promise as a viable option for providing “green” energy to small electrical devices. Calculate for the reaction that takes place in DMFCs: CH 3 OH ( l ) + 3 / 2 O 2 ( g ) → CO 2 ( g ) + 2 H 2 O ( l ) Use values of Δ G f ∘ from Appendix 4.

Chemistry: An Atoms First Approach

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Chemistry: An Atoms First Approach

Direct methanol fuel cells (DMFCs) have shown some promise as a viable option for providing “green” energy to small electrical devices. Calculate for the reaction that takes place in DMFCs:

CH 3 OH ( l ) + 3 / 2 O 2 ( g ) → CO 2 ( g ) + 2 H 2 O ( l )

Use values of Δ G f ∘ from Appendix 4.

Explanation of Solution

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