Answered: Assume the specifications of a Ni-Cd…

Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.29 A of current for 1.00 h. What is the minimum mass (in g) of the cadmium that must be used to make the anode in this cell? AT

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 101E

See similar textbooks

Related questions

Q: (a) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it…

A: Concept introduction: Anodic reaction: It is the reaction that occurs at anode by loss of electrons…

Q: A certain electrochemical cell has for its cell reaction: Zn + HgO → ZnO + Hg Which is the…

A: This question belong to Electrochemistry chapter topic are Galvanic Cell. We have solved this…

Q: A constant current of 1.6 A is used to precipitate copper at the cathode and oxygen at the anode of…

A: value of constant current = 1.6 A Time = 30.4 minutes cathode - copper Anode - oxygen

Q: An electrolytic cell contains inert electrodes in a solution of acidified copper(II) nitrate. Write…

A: Two platinum inert electrodes are dipped in Cu(NO3)2 aqueous solution. One electrode is connected to…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.25 A of current for 1.00 h.…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Sn metal…

A: A electrochemical cell works only when the chemical energy is changed to electric energy. The…

Q: I only need help with the first two questions

A: The relation (1) provides the formula for calculating the electrode potential of a cell and the…

Q: For each of the following Electrochemical cells A and B below: • Write the two half-reactions…

A: "Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Hg metal…

A: Redox reaction - it is also known as oxidation- reduction reaction. It is a type of chemical…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Sn metal…

Q: All WOTK men A solution of NaCl (aq) is electrolyzed for 15.5 min using a current of 3.45 A. Write…

A: Given that, a solution of NaCl (aq) is electrolyzed. The time is t = 15.5 min = (15.5×60) sec = 930…

Q: Draw an electrolytic cell in which Mn2+ is reduced to Mn and Snis oxidized to Sn2+. Label the anode…

A: An electrolytic cell is the electrochemical cell which converts the electrical energy into chemical…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.32 A of current for 1.00 h.…

A: Answer: According to the current value and time duration, charge required is…

Q: During the discharge of an alkaline battery, 4.50 g of Zn is consumed at the anode of the battery.…

Q: An aluminum half-cell is made with 1.00 x 10-3 M Zn(NO3)3 solution and a zinc electrode. A nickel…

A: Since you have asked a question with multiple subparts we will answer the first one for you. To get…

Q: Determine the minimum voltage required to produce l2 (s) in a Mgl2 (aq) cell with inert electrodes.…

Q: Two different electrolytic cells are constructed to electroplate two identical objects based on the…

Q: In an experiment similar to this one, a polished strip of Cu (s) was found to weigh 16.552 g. This…

A: Given : Mass of Cu before electrolysis = 16.552 g Current passed = 0.887 A Time = 26 min = 26 X 60 =…

Q: Calculate the emf for a voltaic cell, constructed from a zinc half-cell and copper half-cell, and…

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.37 A of current for 1.00 h.…

A: Given I = 0.37 A t = 1 hr = 60*60 S Minimum mass of Cadmium = ? g

Q: b.) Write the overall balanced redox reaction occurring in this voltaic cell. How many electrons are…

A: b) 6 electrons being transferred during electrochemical reaction.

Q: Suppose the galvanic cell sketched below is powered by the following reaction: Zn(s)+FeCl,(aq) - -…

A: From the give cell reaction, the balanced equation for the half-reaction that happens at cathode od…

Q: Draw an electrolytic cell in which Mn2+ is reduced to Mn and Sn is oxidized to Sn2+. Label the anode…

A: According to the given data, manganese is taken as cathode and tin is taken as anode so that, when…

Q: A 1.00 g of metal sample took 31.05 minutes to be consumed in the anode to recharge a battery using…

A: According to Faraday's first law of electrolysis, the mass of a substance deposited on the electrode…

Q: Sketch the galvanic cell based on the following overall reactions. Calculate E°; show the direction…

A: For a cell Cell potential = E°Reduction half - E°Oxidation half Species whose reduction potential…

Q: Consider the Nernst equation. A voltaic cell is constructed that uses the following reaction and…

A: No of electrons = 2 2nd term of nernst equation =?

Q: An electrochemical cell is constructed according to the line notationPt | Sn2+ (1.00 M), Sn4+ (1.00…

A: Electrochemistry is the branch of chemistry that studies the change of chemical energy into…

Q: A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M iron(II) ion solution…

A: Oxidation is the process that involved the loss of electrons and oxidized to cation. Hence when a…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Co metal…

A: Interpretation: We have to write the reaction between Co metal and F2(g)

Q: (a) Write the half-reactions predicted to occur at the anode and cathode, based on the standard cell…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Ag metal…

A: Here we have to explain the reaction between Ag metal and Cl2(g). Standard reduction potential of Ag…

Q: Shown in the image is a diagram for the voltaic cell with the overall cell reaction being Al + Pb2+…

A: In the given cell Al electrode is anode because oxidation of Al is taking place while Pb electrode…

Q: Why is a 0 potential possible in electrolysis and not in voltaic cell?

A: The cell potential of any cell is defined as, E∘cell = E∘cathode - E∘anode = E∘reduction…

Q: Use a table of Standard Reduction Potentials to predict if a reaction will occur between Al metal…

Q: Explain how it is possible to make a galvanic cell with a non-zero voltage using the same material…

A: A galvanic cell with a non-zero voltage and that has same material as cathode and anode is termed as…

Q: A half-cell is prepared by immersing a strip of indium metal in a solution containing 1 M In(NO3)3.…

Q: Questions attached

A: Note: Since we solve one question at a time, we’ll answer the first question as the exact one wasn’t…

Q: Sketch the cell, labeling the anode and cathode and indicating the corresponding electrode…

A: #(b): Given the half-cells are Cd(s) rod dipped into a solution of Cd(NO3)2(aq) and Ag(s) rod dipped…

Q: A certain half-reaction has a standard reduction potential Ered=+0.90 V. An engineer proposes using…

A: It is given that E°cell ≥ 0.70 E°cat = 0.90 V

Q: Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.46 A of current for 1.00 h.…

Q: Salt bridge A concentration cell similar to the one shown is composed of two Al electrodes and…

A: Left compartment : anode = oxidation Right compartment : cathode = reduction Anode : Al .....>…

Q: A constant current of 0.800 A was used to deposit copper at the cathode and oxygen at the anode of…

A: The half-reactions that will occur are as follows:

Q: In a hydrogen fuel cell, the steps of the chemical reaction are at -electrode: H2 + 20H-→2H20 + 2e-;…

A: The reaction at each electrode is: Anode H2 + 2OH-→2H2O + 2e-…

Q: For each set of half reactions, write the overall balanced equation for the reaction and calculate…

A: The question is based on the concept of electrochemistry. we have to write the net ionic equation…

Q: A Galvanic cell is consisting of standard concentrations: Cu|Cu2+||Ag+ |Ag, is connected to a small…

A: From the Galvanic cell diagram, the Copper metal is being oxidised to Cu2+ ion Hence the oxidation…

Q: Sometimes in a galvanic cell, an inert electrode is needed. What element is typically used? (Give…

A: Galvanic cell :- An electrochemical cell in which chemical energy of a spontaneous redox reaction…

Q: How do you determine which half-reaction is at the cathode and which at the anode in a voltaic cell?

A: In the electrochemical cell, the chemical energy is converted into electrical energy. The addition…

Q: A half-cell is prepared by immersing a strip of indium metal in a solution containing 1 M In(NO3)3.…

A: Since you have posted questions with multiple sub-parts, we are entitled to answer the first 3 only.…

Question

Assume the specifications of a Ni-Cd voltaic cell include delivery of 0.29 A of current for
1.00 h. What is the minimum mass (in g) of the cadmium that must be used to make the anode in
this cell?

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

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

Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a) Calculate E° for the cell. (b) When the cell operates, what happens to the concentration of Zn2+? The concentration of Sn2+? (c) When the cell voltage drops to zero, what is the ratio of the concentration of Zn2+ to that of Sn2+? (d) If the concentration of both cations is 1.0 M originally, what are the concentrations when the voltage drops to zero?
Consider a voltaic cell in which the following reaction takes place in basic medium at 25°C. 2NO3-(aq)+3S2(aq)+4H2O3S(s)+2NO(g)+8OH(aq) (a) Calculate E°. (b) Write the Nernst equation for the cell E. (c) Calculate E under the following conditions: PNO=0.994atm,ph=13.7,[S2]=0.154M,[NO3-]=0.472M, .
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
A galvanic cell is based on the following half-reactions at 25C: Ag++eAg H2O2+2H++2e2H2O Predict whether is larger or smaller than for the following cases. a. [Ag+]=1.0M,[H2O2]=2.0M,[H+]=2.0M b. [Ag+]=2.0M,[H2O2]=1.0M,[H+]=1.0107M
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.
Consider a salt bridge cell in which the anode is a manganese rod immersed in an aqueous solution of manganese(II) sulfate. The cathode is a chromium strip immersed in an aqueous solution of chromium(III) sulfate. Sketch a diagram of the cell, indicating the flow of the current throughout. Write the half-equations for the electrode reactions, the overall equation, and the abbreviated notation for the cell.
Determine the standard cell potential and the cell potential under the stated conditions for the electrochemical reactions described here. State whether each is spontaneous or nonspontaueous under each set of conditions at 293.15 K. (a) Hg(l)+S2(aq,0.10M)+2Ag+(aq,0.25M)2Ag(s)+HgS(s) (b) The galvanic cell made from a half-cell consisting of an aluminum electrode in 0.015 M aluminum nitrate solution and a half—cell consisting of a nickel electrode in 025 M nickel(l) nitrate solution. (c) The cell made of a half-cell in which 1.0 M aqueous bromide is oxidized to 0.11 M bromine ion and a half-cell in which aluminum ion at 0.023 M is reduced to aluminum metal. Assume the standard reduction potential for Br2(l) is the same as that of Br2(aq).
Atomic masses can be determined by electrolysis. In one hour, a current of 0.600 A deposits 2.42 g of a certain metal, M, which is present in solution as M+ ions. What is the atomic mass of the metal?
Consider a galvanic cell for which the anode reaction is 3 Pb(s)Pb2+(1.0102M)+2e and the cathode reaction is VO2+(0.10M)+2H3O+(0.10M)+eV3+(1.0105M)+3H2O(l) The measured cell potential is 0.640 V. Calculate E for the VO2+V3+ half-reaction, usingE(Pb2+Pb) from Appendix E. Calculate the equilibrium constant (K) at 25°C for thereaction Pb(s)+2VO2+(aq)+4H3O+(aq)Pb2+(aq)+2V3+(aq)+6H2O(l)