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General Chemistry II-Lecture,Section-1-Spring 2025
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The following questions refer to a galvanic cell that utilizes the following reaction (unbalanced):(AuCl4)-(aq) + Cu(s) ® Au(s) + Cl-(aq) + Cu2+(aq)
Determine the number of electrons transferred during the reaction (when balanced).
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The standard free energies of formation of several aqueous species are
What is the standard reduction potential of methanoic acid in aqueous solution (that is, for HCOOH + 4H+ + 4e- ® CH3OH + H2O)?
| kJ/mol | |||
| H+(aq) | 0 | ||
| H2O(l) | -237 | ||
| CH3OH(aq) | -163 | ||
| HCOOH(aq) | -351 | ||
| e- | 0 | ||
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What quantity of charge is required to reduce 31.2 g of CrCl3 to chromium metal? (1 faraday = 96,485 coulombs)
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An excess of finely divided iron is stirred up with a solution that contains Cu2+ ion, and the system is allowed to come to equilibrium. The solid materials are then filtered off, and electrodes of solid copper and solid iron are inserted into the remaining solution. What is the value of the ratio [Fe2+]/[Cu2+] at 25°C?
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A concentration cell is constructed using two Ni electrodes with Ni2+ concentrations of 1.70 M and 4.40 ´ 10-4 M in the two half-cells. The reduction potential of Ni2+ is -0.23 V. Calculate the potential of the cell at 25°C.
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In a common car battery, six identical cells each carry out the following reaction: Pb + PbO2 + 2HSO4- + 2H+ ® 2PbSO4 + 2H2OSuppose that to start a car on a cold morning, 126 amperes is drawn for 13.0 seconds from such a cell. How many grams of Pb are consumed? (The atomic mass of Pb is 207.19 g/mol.)
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If an electrolysis plant operates its electrolytic cells at a total current of 1.0 ´ 106 amp, how long will it take to produce one metric ton (one million grams) of Mg(s) from seawater containing Mg2+? (1 faraday = 96,485 coulombs)
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A solution of MnO42- is electrolytically reduced to Mn3+. A current of 8.14 amp is passed through the solution for 12.4 minutes. How many moles of Mn3+ produced in this process? (1 faraday = 96,485 coulombs)
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Copper is electroplated from an aqueous CuSO4 solution. A constant current of 5.42 amp is applied by an external power supply. How long will it take to deposit 4.06 ´ 102 g of Cu? The atomic mass of copper is 63.546 g/mol.
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Electrolysis of a molten salt with the formula MCl, using a current of 3.86 amp for 16.2 min, deposits 1.52 g of metal. Identify the metal. (1 faraday = 96,485 coulombs)
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