A current of 9.22×10* A is passed through an electrolysis cell containing molten CaCl, for 10.9 days.(a) How many grams of calcium are produced?(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm?

We will use relation of mass and gm equivalent

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 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

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

Which statement is true regarding the galvanic cell in which an electric current is being produced? Zn²* + 2e¯→Zn E° = -0.76 V Cu2* + 2e¯→Cu E° = +0.34 V V Salt Bridge Zn - Cu ZnSO«(aq) CUSO:(aq) (A) Oxidation occurs at the copper electrode. (B) The mass of the copper electrode is increasing. (C) Zinc ions are produced at the copper electrode. (D) Copper ions are produced at the copper electrode.
Nonmetallic phosphorus can be made by the electrolysis of molten P4010. (a) What mass of P is formed by passing a current of 8.60 A through molten P4010 for 1.30 days? The unbalanced chemical reaction representing this electrolysis is shown below. g of P is formed by this electrolysis. (b) How many minutes are needed to plate out 14.00 g of P from molten P4010 using 8.97 A current? minutes are needed. P4010 → P + 0₂
The following figure represents an electrochemical cell at 25.00C with aqueous solutions that behave ideally: (a) Represent the electrochemical cell using cell notation, by taking into account that concentrations of the ZnSO4 and CuSO4 solutions are 0.25 M and 0.35 M, respectively. (b) Calculate the standard potential of the cell, E0cell. (c) Calculate the potential of the cell, Ecell. (d)Calculate DG0 (e)Calculate DG (f)Calculate the equilibrium constant, K.
A 0.04 M sulfuric acid solution was electrolyzed using copper electrodes. A constant current of 4.44 A for 4.2 minutes caused hydrogen gas to be produced at the cathode. Determine the volume of hydrogen gas (in liters, L) produced at 27.8°C and 1.44 atm. |= nF/t F = 96,485 C/mol 1A = 1 C/sec 1V= 1 J/C Do not include units in your answer, If you round during your calculations make sure to keep at least 3 decimal places. Report your answer to three (3) decimal places. Answer: 0.199 The correct answer is: 0.099
To improve conductivity in the electroplating of automo-bile bumpers, a thin coating of copper separates the steel from aheavy coating of chromium. (a) What mass of Cu is deposited on an automobile trim piece ifplating continues for 1.25 h at a current of 5.0 A? (b) If the area of the trim piece is 50.0 cm² , what is the thickness of the Cu coating (d of Cu =8.95 g/cm³)?
Metallic nickel can be made by the electrolysis of molten NiCl₂. (a) What mass of Ni is formed by passing a current of 7.09 A through molten NiCl₂ for 4.70 days? The unbalanced chemical reaction representing this electrolysis is shown below. NiCl₂ → Ni + Cl₂ g of Ni is formed by this electrolysis. (b) How many minutes are needed to plate out 18.00 g of Ni from molten NiCl₂ using 6.93 A current? minutes are needed.
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
An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of 3.00 A passing for 25.0 min. If 1.572 g Ru is produced at the cathode, what is the charge on the ruthenium ions in solution? Charge =|
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?