8. Tunium (Tn) and ciprium (Ci) are two imaginary transition metals used to make a battery. The unbalanced reaction for the battery is given below. Tn(s) + CiO2(s) = Tn0(s) + Ci2O3(s) a. Use the half-reaction method to write a balanced equation for the anode half-reaction, cathode half-reaction, and cell reaction, keeping in mind that the half-reactions occur only in basic solution. Anode: Cathode: Cell: b. A battery is "dead" when the cell reaction reaches equilibrium, which typically occurs when one of the reactants is used up. If the battery initially contains 5.0 g of Tn and 15.0 g CiO2 and discharges at a constant current of 50.0 mA, how many hours before the battery is dead? The molar mass of Tn is 112.66 g/mol and the molar mass of Ci is 123.14 g/mol.

8. Tunium (Tn) and ciprium (Ci) are two imaginary transition metals used to make a battery. The unbalanced reaction for the battery is given below. Tn(s) + CiO2(s) = Tn0(s) + Ci2O3(s) a. Use the half-reaction method to write a balanced equation for the anode half-reaction, cathode half-reaction, and cell reaction, keeping in mind that the half-reactions occur only in basic solution. Anode: Cathode: Cell: b. A battery is "dead" when the cell reaction reaches equilibrium, which typically occurs when one of the reactants is used up. If the battery initially contains 5.0 g of Tn and 15.0 g CiO2 and discharges at a constant current of 50.0 mA, how many hours before the battery is dead? The molar mass of Tn is 112.66 g/mol and the molar mass of Ci is 123.14 g/mol.

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: None

A: a) Electron flow towards the anode: FalseAt the cathode, reduction occurs, representing the gain of…

Q: A chemist designs a galvanic cell that uses these two half-reactions: MnO4(aq) + 2 H₂O(1)+3e Zn²+…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction NO3(aq) + 4 H…

A: The standard reduction potentials for half cell reactions given are NO3– (aq) + 4 H+ (aq) + 3 e–→NO…

Q: <Electrochemistry Exercise 20.79 - Enhanced with Feedback MISSED THIS? Watch KCV: Cell Potential and…

Q: Designing a galvanic cell from tw... A chemist designs a galvanic cell that uses these two…

A: In a galvanic cell , a spontaneous redox reaction Occur . Therefore, the electrode which has a…

Q: A certain half-reaction has a standard reduction potential Ered=-0.70 V. An engineer proposes using…

A: The cell potential needed by the engineer is 1.40 V or greater. The reduction potential of…

Q: Answer the following questions about this cell. Write a balanced equation for the half-reaction that…

A: A Galvanic cell is made up of an anode and a cathode. Reduction reaction occurs at cathode whereas…

Q: A galvanic cell is powered by the following redox reaction: Br₂(1) + H₂(g) + 2OH(aq) 2 Br (aq) + 2…

Q: 9.Given the EoCell for the aluminium –air battery is 2.71 V, what is Eo for the reduction…

A: Given, Standard cell potential of aluminum–air battery = EoCell = 2.71 V What is Eo for the…

Q: Use the given equasion and the Standard Reduction Potentials table to determine which statement is…

A: According to equation 5, the Eocell is given by, => Eocell = Eored (cathode) - Eored (anode)…

Q: Consider a voltaic cell designed to study the redox reaction between Cu²+ and Ni(s). Ni(NO3)2 and…

A: Redox reaction: It is a chemical reaction, where both the oxidation and reduction occur at the same…

Q: A rechargeable battery is constructed based on a concentration cell constructed of two Ag/Ag*…

A: Mole is the amount of the substance that contains the same number of particles or atoms or…

Q: Write the half-cell reaction for the following: a. Pt(s), Cl2 (g), HCl (aq), → HBr (aq), Br2 (l), Pt…

A: Left hand side is written the anode reaction and right hand side is written the cathode reaction.…

Q: A voltaic cell utilizes the following reaction: 4Fe2+(aq)+O2(g)+4H+(aq)→4Fe3+(aq)+2H2O(l) A) E…

A: +

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2 H₂O()+2e 1…

A: Since you have asked multiparts, we will solve the first three subparts for you. If you want any…

Q: The Ni/Cd battery is based on the following overall reaction: Cd(s) + NiO2(s) → CdO(s) + NiO(s)…

A: Cell reaction : Cd(s) + NiO2(s) → CdO(s) + NiO(s) Oxidation reaction is…

Q: Write the reduction half-reaction for the corrosion of iron. Express your answer as a half-reaction…

A: Electrolysis is used to plate metal over the another metal surface.

Q: 4. *For the unbalanced reaction Fe3+(aq) +I-(aq) → Fe²*(aq) + I2(s) Balance the reaction and label…

A: Basic terms: Anode: It is an electrode at which the oxidation half-reaction occurs. Cathode: It is…

Q: Consider a galvanic cell consisting of the Cr3+/Cr (Eo=-0.74 V) and the Ag+/Ag (Eo=+0.8 V) systems…

A: Since the reduction potential of Cr3+/Cr is more negative than Ag+/Ag, Cr will reduce Ag+ to Ag.…

Q: A voltaic cell with a basic aqueous background electrolyte is based on the oxidation of Cd(s) to…

A: The voltaic cell is based on the oxidation of Cd (s) to Cd(OH)2 (s) and the reduction of MnO4− to…

Q: O₂(g)+4 H (aq)+4e 2 H₂O(1) 3+ 2+ Fe (aq)+e → Fe (aq) Write a balanced equation for the half-reaction…

A: We will see the reduction potential of both electrode reactions. the electrode which has more…

Question

100%

8. Tunium (Tn) and ciprium (Ci) are two imaginary transition metals used to make a battery. The
unbalanced reaction for the battery is given below.
Tn(s) + CiO2(s) = TnO(s) + Ci2O3(s)
a. Use the half-reaction method to write a balanced equation for the anode half-reaction, cathode
half-reaction, and cell reaction, keeping in mind that the half-reactions occur only in basic solution.
Anode:
Cathode:
Cell:
b. A battery is "dead" when the cell reaction reaches equilibrium, which typically occurs when one of
the reactants is used up. If the battery initially contains 5.0 g of Tn and 15.0 g CiO2 and discharges
at a constant current of 50.0 mA, how many hours before the battery is dead? The molar mass of
Tn is 112.66 g/mol and the molar mass of Ci is 123.14 g/mol.

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

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 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

Please answer all parts.
An electrochemical cell uses Ag and Zn as electrodes. Based on the reduction potentials, the (blank) electrode is where the reduction will occur and it is called the (blank) a.Ag, cathode b.Zn, anode c.Ag, anode Based on the reactions below, which is the stongest reducing agent? +1.22 V MnO2(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H2O(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2- (aq) -0.95 V SnO2(s) + 2H2O() + 4e-→ Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- → Cr(s) + 3OH-(aq) a.Hg2SO4 b.Mn02 c.Cr d.Sn e.Hg Identify the strongest oxidizing agent from the following half-reactions. The standard reduction potentials are listed. +1.22 V Mn02(s) + 4H+(aq) + 2e- → Mn2+(aq) + 2H20(1) +0.61 V Hg2SO4(s) + 2e- → 2Hg(1) + SO4 2-(aq) -0.95 V SnO2 (s) + 2H2O() + 4e- Sn(s) + 40H-(aq) -1.48 V Cr(OH)3(s) + 3e- Cr(s) + 3OH- (aq) a. MnO2 b.Hg2SO4 c.Sn d.Hg e.Cr
*Please write the half-reactions for the anode and cathode and explain if you can. Thank you in advance* Consider the electrolysis of aqueous solutions below. For each, show the species produced at the anode and the cathode. Aqueous FeCl3.
Given the following half cells: Fe2+/Fe0 and Pd/Pd2+, determine; a) what is the anode and what is the cathode, b) what is Eo, c)what is Go and k? Using the following concentrations, determine E value for your cell. Fe2+ [.25], Pd2+ [.05]. How long would you have to run this battery at 3.2 amps to lower the E by .05 volts?
8. Identify the half reactions that occur in an electrolytic cell consisting of copper electrodes in a solution of CrBr,.
QUESTION 1 Match the following terms to the correct definition. standard reduction potential (E°) Anode Cathode oxidation half-reaction Galvanic cell Cell potential reduction half-reaction electrical potential - A. difference in electrical potential that arises when dissimilar metals are connected; the driving force for the flow of charge (current) in oxidation-reduction reactions B. "the half of an oxidation-reduction reaction involving oxidation; the half-reaction in which electrons appear as products; balanced when each atom type, as well as the charge, is balanced" C. electrode in an electrochemical cell at which oxidation occurs; information about the anode is recorded on the left side of the salt bridge in cell notation D. electrochemical cell that involves a spontaneous oxidation-reduction reaction; electrochemical cells with positive cell potentials; also called à voltaic cell E. "energy per charge; in electrochemical systems, it depends on the way the charges are distributed…
Consider the reaction between solid aluminum, Al and copper ions Cu^2+, to give aluminum ions Al^3+, and solid copper, Cu in an acidic solution. a) write the reduction half cell reaction and find Ered b) Write the oxidation half cell reaction and find Eox c) Write the balanced redox reaction in an acidic solution and find E d) Calculate E if all the ionic species have a concentration of .2 M
need help with this chemistry
For a Magnesium-Aluminum cell [Mn2+ + 2e- --> Mn (-1.18V)] [Al3+ + 3e- --> Al (-1.66)]: 1. label anode, cathode2. write half reactions3. Write overall reaction4. Write cell notation5. Calculate E6. Calculate G = -nFe7. Show and give example of how G is related to K8. Calculate Nernst for various Molarity changes (show how E changes)9. Calculate grams at cathode for different amounts of time