Problem # 1 The fuel cell produces energy based on the reduction reaction of hydrogen, which in turn reacts with oxygen from air to produce water vapor. The reaction set is as follows: Net: H2 + ½ O2 → H2O What is the amount of hydrogen for the fuel cell to provide 500 watts of power with a total voltage of 48 V if it operates at 35% efficiency at full load? What is the amount of air required?

Problem # 1 The fuel cell produces energy based on the reduction reaction of hydrogen, which in turn reacts with oxygen from air to produce water vapor. The reaction set is as follows: Net: H2 + ½ O2 → H2O What is the amount of hydrogen for the fuel cell to provide 500 watts of power with a total voltage of 48 V if it operates at 35% efficiency at full load? What is the amount of air required?

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 certain half-reaction has a standard reduction potential E=+0.21 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.30 V of electrical power. The cell will operate under standard conditions. l Data Note for advanced students: assume the engineer requires this half-reaction to happen at t Half-Reaction E° (V) Ag+ (aq) + e + Ag (s) A13+ (aq) + 3e - Al (s) Au+ (aq) + e - Au (s) Au3+ (aq) + 3e - Au (s) 0.7996 -1.676 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? O yes, there is a minimum. E = Ov 1.692 1.498 If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Ba2+ (aq) + 2e- - Ba (s) -2.912 O no minimum Br2 (1) + 2e - 2Br (aq) 1.066 Ca2+ (aq) + 2e-- Ca (s) -2.868 Cl2 (g) + 2e - 2CI (aq) Co2+ (aq) + 2e-- Co (s) Co3+ (aq) + e - Co2+ (aq) Cr2+ (aq) + 2e → Cr (s) Cr3+ (aq) + 3e +…
The two redox half reactions represented below are combined to create a galvanic cell. Which statements are true regarding this cell? Select all that apply. 2 H+ (aq) + 2 e= H₂(g) Eº = 0.00 V La³+ (aq) + 3 e La(s) Eº = -2.38 V Three electrons are transferred in the overall, balanced reaction for the cell. La³+ is reduced to La(s) at the cathode. The overall, standard cell potential is 2.38 V. La³+ is produced at the anode. H₂(g) is produced at the cathode. La(s) is the oxidizing agent.
Constants The following values may be useful when solving this tutorial. Constant Cu Eco R F T Value 0.337 V -0.277 V 8.314 J. mol-¹.K-¹ 96,485 C/mol 298 K
15 Write the balanced equation for the voltaic cell in basic conditions with the following components (see earlier problem): PbO2, Pb2*, Cr20,2", Cr3+
If the following electrochemical cell is constructed, what voltage will be measured on the voltmeter? Half-Reaction E° (V)   Zn2+(aq) + 2e–→ Zn(s) –0.76     Ag+(aq) + e–→Ag(s) +0.80   Question 6 options: -0.04 V 0.04 V 2.36 V 1.56 V -2.36 V
A voltaic cell consists of a standard hydrogen electrode in one half-cell and a Cu/Cu2+ half-cell. Calculate [ Cu2+ ] when E cell is 0.210 V. × 10 M Enter your answer in scientific notation.
Help with only the last question please explain and breakdown the calculation How many grams of magnesium chloride are produced if a constant current of 25 A is passed through the solution for 1.5 hours?
Consider an electrochemical cell involving Barium and Copper. Ba2+(aq) + 2e- → Ba(s) Eo = -2.92 V Cu2+(aq) + 2e- → Cu(s) Eo = +0.340 V What is the potential of this cell under standard conditions? Answer 1Choose...3.26 V-2.92 VBaCu2.92 VCu to BaBa to Cu2.58 V-0.340 V0.340 V-3.26 V What is the standard reduction potential of Barium (Ba)? Answer 2Choose...3.26 V-2.92 VBaCu2.92 VCu to BaBa to Cu2.58 V-0.340 V0.340 V-3.26 V In the wire, which way do the electrons flow? Answer 3
Suppose you set up an electrochemical cell. In one beaker, you have a 1 M copper(I) ion solution with a copper metal electrode. You use an external wire to connect the cop electrode to an aluminum electrode in another beaker with a 1 Maluminum lon solution. Then you add a salt bridge with sodium sulfate ions. All things are in place to have functional cell. Which of the following statements is FALSE? Nothing will happen until you add an external power source. Without a power source, electrons will travel from the aluminum beaker to the copper beaker You can run this as a voltaic cell and get out a maximum of 2.00 V You can run this as an electrolytic cell only if you input a minimum of 2.00v
Balance the following skeleton reaction, calculate E 0 AgCl(s) + NO(g) → Ag(s) + Cl(aq) + NO3(aq) Balanced reaction: 15 cell This reaction is spontaneous This reaction is nonspontaneous and state whether the reaction is spontaneous. cell' [acidic]
O ADVANCED MATERIAL Analyzing a galvanic cell A galvanic cell is powered by the following redox reaction: 2+ NO3(aq) + 4H+ (aq) + 3 Fe²+ (aq) NO(g) + 2 H₂O(l) + 3 Fe³+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. ローロ Write a balanced equation for the half-reaction that takes place at the cathode. e Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. E = v x