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(1) + 3/2 O2(g) → CO2(g) + 2 H2O(1) Use the following values. AG°H,O(1) =-237 kJ/mol AG°O,(g) = 0 kJ/mol AG°CO,(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(1) + 3/2 O2(g) → CO2(g) + 2 H2O(1) Use the following values. AG°H,O(1) =-237 kJ/mol AG°O,(g) = 0 kJ/mol AG°CO,(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

Topics: Fundamentals of electrochemistry; Electrochemical cells Use general chemistry rules for significant figures. 1. A cell is constructed to reduce the Ag+ in AgCl(s) to Ag(s) at the cathode when current is passed through the cell. At the anode, Cu(s) is oxidized to Cu2+. If current of 0.500 A is passed through the cell for 101 minutes, calculate the mass of Cu(s) dissolved and mass of Ag(s) deposited. Half-cell reactions: Cathode: AgCl(s) + e ⇌ Ag(s) + Cl– Anode: Cu(s) ⇌ Ce2+ + 2e
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
The (fictional) metal unobtanium, Ub, has E° = −0.61 V for the reaction: Ub2+(aq) + 2 e− → Ub(s) a) If the galvanic cell shown below is spontaneous, which metal would be oxidized, and which would be reduced? How do you know? Support your answer with the half-reactions and E°cell. b) Write the overall reaction for this galvanic cell in cell notation.
Consider the following galvanic cell: E° (V) U3+ + 3 e− → U(s) −1.642 In3+ + 2e− → In+ −0.444 What is the anode? In3+/In+ U/U3+ Pt/In3+ Pt/In+
A galvanic cell is prepared using copper and silver. Its cell notation is shown below: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode? A. Cu(s) → Cu2+(aq) + 2e- B. Cu2+(aq) + 2e- → Cu(s) C. Ag+(aq) + e- → Ag(s) D. Ag(s) → Ag+(aq) + e- E. Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) Copper is electroplated from a CuSO4 solution. A constant current of 4.54 A is applied by an external power supply. How long (minutes) will it take to deposit 0.985 g of Cu? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3) DOnt need work shown just answer asap Predict the sign of ΔSorxn (positive or negative) for the following reactions: CH3OH(l) → CH3OH(s) CH4(g) + H2O(g) → CO(g) + 3…
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
Write the cell notation for an electrochemical cell consisting of an anode where Ni (s) is oxidized to Ni2+ (aq) and a cathode where Cu2+ (aq) is reduced to Cu (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
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