Which of your group’s cells do you think would produce the largest voltage? Why?
A promising technology based on a
a. Assign oxidation states to each atom in the reaction.
b. Determine what is being oxidized and what is being reduced.
c. Write and balance the separate half-reactions. (Hint: Methanol reacts to form carbon dioxide, and oxygen reacts to form water.)
d. Balance the overall reaction if it occurs in acidic solution.
e. Methanol fuel cells must be designed to allow
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INTRO TO CHEMISTRY CUSTOM
- An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?arrow_forwardConsider a battery made from one half-cell that consists of a capper electrode in 1 M CuSO4 solution and another half—cell that consists of a lead electrode in 1 M Pb(NO3)2 solution. (a) What are the reactions at the anode, cathode, and the overall reaction? (b) What is the standard cell potential for the battery? (c) Most devices designed to use dry-cell batteries can operate between 1.0 and 1.5 V. Could this tell he used to make a battery that could replace a dry-cell battery? Why or why not. (d) Suppose sulfuric acid is added to the half—cell with the lead electrode and some PbSO4(s) forms. Would the cell potential increase, decrease, or remain the same?arrow_forwardManganese may play an important role in chemical cycles in the oceans. Two reactions involving manganese (in acid solution) are the reduction of nitrate ions (to NO) with Mn2+ ions and the oxidation of ammonium ions (to N2) with MnO2. (a) Write balanced chemical equations for these reactions (in acid solution). (b) Calculate Ecell for the reactions. (One half-reaction potential you need is for the reduction of N2 to NH4+, E = 0.272 V.)arrow_forward
- Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?arrow_forwardA voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?arrow_forwardFor the cell: Cr|Cr3+Co2+|Co E° is 0.46 V. The same cell was prepared in the laboratory at standard conditions. The voltage obtained was 0.40 V. A possible explanation for the difference is (a) the surface area of the chromium electrode was smaller than the cobalt electrode. (b) the mass of the chromium electrode was larger than the mass of the cobalt electrode. (c) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (d) the concentration of Cr(NO3)2 solution used was less than 1.0 M. (e) the volume of Cr(NO3)2 solution used was larger than the volume of Cr(NO3)2 solution used.arrow_forward
- Consider the concentration cell in Fig. 17-10. If the Fe2+ concentration in the right compartment is changed from 0.1 M to 1 107 M Fe2+, predict the direction of electron flow, and designate the anode and cathode compartments.arrow_forwardThe specifications for a lead storage battery include delivery of a steady 1.5 A of current for 15 hours. (a) What is the minimum mass of lead that will be used in the anode? (b) What mass of PbO2 must be used in the cathode? (c) Assume that the volume of the battery is 0.50 L. What is the minimum molarity of H2SO4 necessary?arrow_forward
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