Calculate the amount of Cu (in grams) produced in 1.0 h at inert electrodes in a solution of CuBr2 by a current of 4.50 A. (MMCU = 63.55 g/mol) Cu2*(aq) + 2e → Cu(s) 2Br (aq) → Br2(1} + 2e 13.4 g O 21.7 g 9.35 g O5.35 g

Calculate the amount of Cu (in grams) produced in 1.0 h at inert electrodes in a solution of CuBr2 by a current of 4.50 A. (MMCU = 63.55 g/mol) Cu2*(aq) + 2e → Cu(s) 2Br (aq) → Br2(1} + 2e 13.4 g O 21.7 g 9.35 g O5.35 g

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

Related questions

Q: A total of 1.740 F of electricity (1 F=1 mol e−) was required to electrodeposit all of the Zn and Co…

A: The mass of each compound is calculated by the number of moles of the compound. The number of moles…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2V0; (aq) +…

A: = 7.43 M[H+] = 1.74 M[VO2+] = 5.87 M[Fe2+] = 5.04 MT = 25oC=25+273=298Kn=2 as 2 electrons are…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.68 minutes for a current of 1.08 A to plate…

A: The metal will come out as M3++3e-= M . We can conclude from here that 3 moles of electrons are…

Q: Silver can be electroplated at the cathode of an electrolysis cell according to the following…

A: Given information:Current (I) = 6.4 ATime (t) = 69 minutes

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for…

A: According to the Faraday's first law of electrolysis, the amount of any substance deposited at the…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2103 (aq)…

A: The question is based on the concept of electrochemistry . we need to calculate cell potential of…

Q: How long in seconds would it take to deposit 59.07 g of Pt from an aqueous solution of Pt 2+ with a…

Q: How long must a current of 20.0 amps be applied to a solution of CrCl3 to produce 175 g of Cr (s)…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

Q: Copper is electroplated from CuSO4 solution. A constant current of 4.28 A is applied by an external…

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: According to Faraday's Law: W=ZIt ...... (1) where w is the mass formed, I…

Q: What mass of zinc (in grams) is deposited at the cathode when a current of 9.8 amperes passes…

A: According to the electrochemistry Mass of substance deposited, W = ZCt Where, t = time in second…

Q: How many minutes will it take to electroplate 32.1 gg of gold by running 5.00 AA of current through…

A: Au+ + e- ------> Au 1 mol of Au requires 1 mol of electron 1 mol of electron = 96485 C…

Q: How long (in hours) must a current of 4.61 amps be passed to produce 79.5 g of copper metal from a…

A: Given:: Current i= 4.61 A Mass of Cu = 79.5 g Molar mass of Cu= 63.55 g mol-1 Time t= ?

Q: Determine the molar mass (amu) of Metal (M) if it took 1.04 minutes for a current of 1.22 A to plate…

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: In electrolysis cation is attracted towards cathode and anion is attracted towards to the anode.

Q: an irregularly shaped metal part was made from a particular alloy was galvanized with zinc using a…

A: Given The amount of current (I) is 2.15 A The time is 2.2 hours The density of zinc is 7.410 g/cm3…

Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

A: 1 F = 96500 C Moles of chlorine = 1090 / 71 = 15.35 moles Total charge = 2 × 15.35 F = 2 × 15.35…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2+ 2 Cr³+…

A: In an electrochemical cell, the chemical energy due to the chemical reactions is converted into…

Q: A Cr3+1aq2 solution is electrolyzed, using a current of 7.60 A. What mass of Cr(s) is plated out…

A: Charge flowing per unit time is known as current which may be expressed mathematically as :…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3 Cu²+…

Q: In the electrolysis of an acid solution, oxygen can be produced by the following half-reaction:…

Q: Determine the molar mass (amu) of Metal (M) if it took 2.85 minutes for a current of 1.1 A to plate…

A: Molar mass can be calculated as:-

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

A: Step 1: Calculate the cell voltage, using the Nernst equation. Ecell = E°cell - (RT/nF)lnQ where:-…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: Sn²+ (aq)…

A: Given Cell reaction: Sn2+(aq) + Ba (s)---> Ba2+(aq) + Sn (s) From standard electrochemical data,…

Q: Aluminum(III) ion (Al 3+) is reduced to solid aluminum at an electrode. If a current of 2.75 amperes…

Q: What volumes of H₂(g) and O₂(g) at STP are produced from the electrolysis of water by a current of…

A: Given ,

Q: A metal was galvanized with zinc using a solution of zinc nitrate, Zn(NO3)2. How much time was…

A: Answer : We have to calculate time to plate zinc on the metal . Using Faraday laws of electrolysis…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq) +…

A: Oxidation is lose of electrons. Reduction is gaining of electrons. Galvanic cell is an…

Q: Determine the molar mass (amu) of Metal (M) if it took 1.29 minutes for a current of 1.48 A to plate…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 210, (aq) +…

Q: An aqueous copper (II) chloride solution is electrolyzed for a period of 156 minutes. Using a…

A: We have given that An aqueous copper (II) chloride solution is electrolyzed for a period of 156…

Q: Chromium can be plated from solution of CrCl3(aq) according to the following half reaction. How many…

Q: (a) A student is required to construct a battery in the form of a galvanic cell using nickel (II)…

Q: Electrolytic process of determining molar mass. An electrolysis cell contains X3+ ions. When a 5.45…

A: In a electrolytic process, cations go to the anode and anions go to the cathode.

Q: What constant current would be needed for a copper cathode to accumulate 3.06 g of copper in 30 min.…

A: given- mass = 3.06 g. time = 30 min = 30 x60 = 1800 sec electrochemical equivalent of copper = 3.29…

Q: This is an example of a disproportionation reaction:…

Q: (a) A student is required to construct a battery in the form of a galvanic cell using nickel (II)…

A: The reduction potential of Nickel(-0.40v) is less than that of cadmium(-0.26v) , hence Nickel will…

Q: A galvanic cell is constructed using the following half-reactions at 298 K. Given Kf = 1.0 x 10^8…

A: Given formation constant for MX42+(aq) , Kf = 1.0*108 Since Kf >> 1, formation of MX42+(aq)…

Q: Chlorine, Cl2, is produced commercially by the electrolysis of aqueous sodium chloride. The anode…

Q: Electrolytic process of determining molar mass. An electrolysis cell contains X3+ ions. When a 5.45…

A: Given: Current=5.45A Time=2.16×103s Mass of the element=8.50 g To find: Molar mass of X

Q: Determine the amount of time (in hours) that a 16.8 ampere current must be applied to a 2.0…

A: The objective of the question is to find out the time required to produce a certain amount of Zinc…

Q: Calculate the amount of Cu (in grams) produced in 1.0 h at inert electrodes in a olution of CuBr2 by…

A: From faraday's law of electrolysis, W = Zit = Eit/F Z = E/F Where , w is the mass deposit on…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq)…

A: Step 1: Step 2: Step 3: Step 4:

Q: A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl₂ for…

Q: A certain electrolytic cell produced 39.0 g Cl, from molten NaCl. The time it took for this process…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Calculate the armount of Cu (in grams) produced in 1.0 h at inert electrodes in a
solution of CuBr2 by a current of 4.50 A.
(MMCu = 63.55 g/mol)
%3D
Cu2*(aq) + 2e → Cu(s)
2Br (aq} → Br2(1} + 2e
O 13.4 g
O 21.7 g
9.35 g
5.35 g

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1 : Given

VIEW

Step 2 : Explanation

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

75. Which of the following statements associated with the pH meter is incorrect? (A) The pH meter should include a working electrode, a reference electrode, and a counter electrode. (B) The pH meter is unable to determine the pH of 0.1 M NaOH. (C) Silver chloride-coated silver wire is commonly used as a reference electrode in the pH meter. (D) The glass membrane must be hydrated. (E) The difference in potential between the inner and outer layers is the boundary potential.
G ロ・ロ A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3+ MnO2 (s) + 4H* (aq) +2Cr²* (aq) → Mn²* (aq) + 2H2O (1) +2Cr³+ (aq) Suppose the cell is prepared with 0.190 M H* and 6.41 M Cr²+ in one half-cell and 0.205 M Mn2+ and 1.94 M Cr3+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ ☐ x10 μ
Chromium can be electroplated from aqueous potassium dichromate, with the reduction shown below. If a current of 5 A and a voltage of 4.5V are used: Cr20, (aq) + 14H+ (aq)+ 12e¯ → 2Cr(s) + 7H20 How many hours would it take to completely convert 215 mL of 1.11 M K2Cr207 to elemental chromium?
what mass, in g, of copper will be deposited from a solution of Cu^2+ by a current of 2.43 A in 7.52 h?
A typical 12-ounce aluminum beverage can weighs 12.5 grams. Suppose you consume an average of three 12-ounce beverages a day (in the Al can) for an entire year. How many hours will it take to manufacture the needed aluminum using an electrolysis cell supplied with a 150-amp current? The reaction used to make the Al metal is 2A12O3(1) + 3C(graphite) → 3CO2(g) + 4Al(1)
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 2103 (aq) +12H* (aq) + 5Co (s) → 1₂ (s) + 6H₂O (1) +5Co²+ (aq) 2+ Suppose the cell is prepared with 5.23 M IO3 and 2.31 M H in one half-cell and 6.84 M Co in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
The deuterated ethanol shown can be converted to an alkyl halide via a mesylate intermediate. Complete the mechanism, draw the final product (with nonbonding electrons) and select the correct absolute stereochemistry of the starting material and the final product.
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3+ 2+ 2 Cr³+ (aq) + 3Ca (s) → 2Cr (s) + 3 Ca²+ (aq) 3+ 2+ Suppose the cell is prepared with 2.68 M Cr in one half-cell and 7.85 M Ca in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 ロ・ロ × μ 0|0 Ś
Help with the following question Please round the answer to 3 sig figs
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210, (aq) + 12H" (aq)+ 5Co (s) → L, (s)+ 6H,0 (1)+ 5Co" (aq) Suppose the cell is prepared with 6.10 M IO, and 1.61 M H' in one half-cell and 7.06 M Co 2+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. х10
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3 Cu²+ (aq) + 2Al(s) → 3Cu (s) +2A1³+ (aq) 2+ Suppose the cell is prepared with 4.04 M Cu²+ in one half-cell and 4.43 M A1³+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 X 3 8 Ś
How many grams of X (MW = 91.45 g/mol)(in g) will be deposited on a cathode in 1.15 h by a current of 4.0 A? X6+ + 6e- → X(s) Report your answer with the correct number of significant figures.