A current of 9.22×104 A is passed through an electrolysis cell containing molten CaCl, for 10.9 days. (a) How many grams of calcium are produced? |g (b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1 L

A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.

Consider the following galvanic cell: Cu(s) | Cu²+ (aq) || Ag+(aq) | Ag(s) Identify the cathode and state if it is being oxidized or reduced (please refer to chart on reference data page.) (A) Cu is the cathode; it is being oxidized (B) Cu is the cathode; it is being reduced (C) Ag is the cathode; it is being oxidized (D) Ag is the cathode; it is being reduced (E) Since the E values for both Ag and Cu are positive, they are both cathodes and being reduced

I need the solution (with work) for D

O ELECTROCHEMISTRY = Understanding concentration cells ODDOD 3/5 A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of MNO3 and the right half cell with a 150. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? Oleft right ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

(a) A silver wire is placed in a solution of CuCl₂. Does this reaction occur under standard conditions? O The reaction occurs. No reaction occurs. (b) Cl2 gas is bubbled into a solution of Nal. Write a balanced net-ionic equation. (Use the lowest possible coefficients. Specify states such as (aq) or (s). If a box is not needed, leave it blank.) 21 (aq) +C1₂(g) Calculate E, AG, and K. E = 0.82 AG = -158.235 K =7.345x10^13 →2Cl(aq) + 1,(s) The reaction occurs. O No reaction occurs. V kj Does this reaction occur, under standard conditions?

B) Balance the following redox reaction in acidic solution: I03 - (aq) + NO2(g) → NO3 (aq) + I»(s)

Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be performed at a current of 2.67 A in order to produce 15.1 g Ca?