Direct methanol fuel cells (DMFCS) have shown some promise as a viable option for providing "green" energy to small electrical devices. Calculate E° for the reaction that takes place in DMFCS: CH3OH() + 3/2 O2(g) → CO2(g) + 2 H2O(1) Use the following values. AG°H,0(1) = -237 kJ/mol AG°O¿(g) = 0 kJ/mol AG°CO2(g) =-394 kJ/mol AG°CH3OH(1) = -166 kJ/mol. E° V

Direct methanol fuel cells (DMFCS) have shown some promise as a viable option for providing "green" energy to small electrical devices. Calculate E° for the reaction that takes place in DMFCS: CH3OH() + 3/2 O2(g) → CO2(g) + 2 H2O(1) Use the following values. AG°H,0(1) = -237 kJ/mol AG°O¿(g) = 0 kJ/mol AG°CO2(g) =-394 kJ/mol AG°CH3OH(1) = -166 kJ/mol. E° V

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...

See similar textbooks

Similar questions

For the galvanic (voltaic) cell 2+ - Fe(s) + Mn²+ (aq) → Fe²+ (aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²+] if [Mn²+] = 0.090 M and E = 0.78 V? Assume T is 298 K 1 4 7 +/- 2 LO 5 8 0.196 M 3 6 9 O X C x 100
In the electrolysis of a sodium chloride solution, what volume of Ch (g) is produced in the same time it takes to produce 6.0 L of H2(g), both volumes measured at 0 °C and 1.0 atm?
A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 2.00 M solution of M₂SO4 and the right half cell with a 10.0 mM solution of the same substance. Electrodes made 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. Which electrode will be positive? 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. V left right x10 X T
Given the balanced electrochemical reaction below (M and N represent generic metals), what is the standard cell potential (E°cell), in volts, for the reaction? Enter your answer to the thousandths place. Do not include units. 2M+(aq) + N(s) → 2M(s) + N2+(aq) ΔG°rxn = -169.0 kJ/mol
3. Calculate the free energy, AG°, for each electrochemical cell given the following information and determine if the reaction is spontaneous or nonspontaneous. T= 298 K a. E cell =+ 2.10 V, n= 2 b. Каg— 2.2 х 10-3 c. E cell =- 0.677 V, n = 3 =
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
thermodynamics
Consider the following galvanic cell: E° (V) U3+ + 3 e− → U(s) −1.642 In3+ + 2e− → In+ −0.444 What is the cathode? U/U3+ In3+/In+ Pt/In3+ Pt/In+
A silver oxide–zinc cell maintains a fairly constant voltage during discharge (1.60 V).The button form of this cell is used in watches, hearing aids, and other electronic devices.The half-reactions are:Zn(s) + 2OH- (aq) → Zn(OH)2(s) + 2eAg2O(s) + H2O(l) + 2e- → 2Ag(s) + 2OH(aq)(a) Identify the anode and the cathode reactions.(b) What’s the overall reaction in this galvanic cell?
Consider the following galvanic cell: E° (V) U3+ + 3 e− → U(s) −1.642 In3+ + 2e− → In+ −0.444 The electron flow is clockwise electrons don't move in this galvanic cell counterclockwise
The electrolysis of SnCℓ4 at high temperature produces tin metal. If a constant electricalcurrent of 15.00 × 103 ?? flows for exactly two hours, calculate the number of tin atomspresent in the metal produced during this time.
Calculate the cell voltage at 25°C for this cell when [H+] = [HSO4–] = 4.5 M. At 25°C, E° = 2.04 V for the lead-acid battery. For this reaction, ∆H° = –315.9 kJ and ∆S° = 263.5 J/mole K. Calculate E° at –20° C and Ecell when [H+] = [HSO4–] = 4.5 M.