3. Application of AG to fuel cells We often associate AG with the idea of equilibrium. We will explore this relation in the next lectures. In this problem, let us briefly explore another interpretation of AG, i.e. how it relates to non-PV work. Suppose you are constructing a fuel cell i.e. a device that converts chemical energy into electrical work. Calculate the maximum amount of electrical work that can be extracted on a per mole basis if the fuel cell is run on the combustion of methane at T = 298 K and P = 1 bar. Assume that the products of combustion, i.e. reaction with oxygen gas, are carbon dioxide gas and liquid water. Note the following values: AH°c(CH4(g)) = -891 kJ mol-¹ and 5°(CO₂(g)) = 213.8 J mol¹¹ K¹¹, S°(H₂O(l)) = 70.0 J mol¹¹ K-¹, S°(CH4(g)) = 186.3 J mol¹¹ K´¹, and Sºᵒ(O₂(g)) = 205.2 J mol-¹ K-¹.

3. Application of AG to fuel cells We often associate AG with the idea of equilibrium. We will explore this relation in the next lectures. In this problem, let us briefly explore another interpretation of AG, i.e. how it relates to non-PV work. Suppose you are constructing a fuel cell i.e. a device that converts chemical energy into electrical work. Calculate the maximum amount of electrical work that can be extracted on a per mole basis if the fuel cell is run on the combustion of methane at T = 298 K and P = 1 bar. Assume that the products of combustion, i.e. reaction with oxygen gas, are carbon dioxide gas and liquid water. Note the following values: AH°c(CH4(g)) = -891 kJ mol-¹ and 5°(CO₂(g)) = 213.8 J mol¹¹ K¹¹, S°(H₂O(l)) = 70.0 J mol¹¹ K-¹, S°(CH4(g)) = 186.3 J mol¹¹ K´¹, and Sºᵒ(O₂(g)) = 205.2 J mol-¹ K-¹.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e 2 Br (aq) :+1.065 V (red Cro, (aq)+4 H,O(1)+3e Cr(OH)3(s)+5 OH (aq) -0.13 V (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode.
For a particular reaction in a galvanic (voltaic) cell ΔS° is negative. Which of the following statements is true? a. ΔG° > 0 for all temperatures. b. ε will decrease with an increase in temperature. c. ε will not change when the temperature increases. d. ε will increase with an increase in temperature. e. None of these choices statements is true.
2. Tell whether each of these statements are true and false. If false, rewite it to make it a correct statement. Oxidation always occurs at the anode of an electrochemical cell. The anode of a voltaic cell is the ite of reduction and is negative. Standard conditions for electrochemical cells are a concentration of 1.0 M for disolved species and a pressure of 1 bar for gases. The potential of a voltaic cell does not change with temperature. All product-favored oxidation-reduction reactions have a standard cell voltage E°cell, with a negative sign.
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ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.96 minutes for a current of 1.62 A to plate 0.0534 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
Based on the sign of the standard cell potential, Eel, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Pb2*(aq) + H2(g) - Pb(s) + 2 H*(aq) Ni?*(aq) + s? (aq) Ni(s)+S(s) Al3+(aq) + 3 Na(s) → Al(s) + 3 Na*(aq)
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.62 minutes for a current of 1.79 A to plate 0.0731 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.14 minutes for a current of 1.97 A to plate 0.0672 g of metal from a solution containing M2(S04)3 (Round off the final answer to TWO decimal places. Do not include the unit.) A Moving to another question will save this response. «< Question 6 of 12 »
Which of the following is not correct ? Electrode potential or cell potential is an intensive property .a O If half reaction is multiplied by a numerical factor, the corresponding Eo value is also multiplied by the same .b O factor. Gibbs energy is an extensive property .c O Electrical work = - AG .d O
A certain metal M forms a soluble nitrate salt M(NO,).. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.00 M solution of M (NO,), and 2 the right half cell with a 150. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. O left x10 Which electrode will be positive? right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.
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