A voltaic cell consists of Co I Co?²*(0.25 M) II Cu²*(0.35M) I Cu. The electrode potential at this concentration is [A] 0.6157V [B] 0.6025 V [c]0.6243V [D] 0.5014 V (Co* + 2 e→ Co, ɛ°red = -0.28 V, Cu²* +2 e→ Cu, ɛ°red = +0.34 V) A C O D

A voltaic cell consists of Co I Co?²(0.25 M) II Cu²(0.35M) I Cu. The electrode potential at this concentration is [A] 0.6157V [B] 0.6025 V [c]0.6243V [D] 0.5014 V (Co* + 2 e→ Co, ɛ°red = -0.28 V, Cu²* +2 e→ Cu, ɛ°red = +0.34 V) A C O D

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: Consider the following cell: |Zn (s) | Ca2* (aq) , so3²" (aq) || Hg2+ (aq) , F° (aq) | Pt (s) | a)…

A: In a cell notation, the left side represent anode reaction or oxidation-half reaction, and the right…

Q: For a standard voltaic cell comprised of a Cu2+|Cu electrode and a Fe3+|Fe2+electrode, what is the…

A: In voltaic cell, a spontaneous reaction occur. Greater the value of standard reduction potential of…

Q: For the cell reaction, Zn(s) | Zn2+(aq, 1 M) || Cu2+(aq, 1 M) | Cu(s), the electrode potential of…

A: In the given question we have to calculate the cell potential. cell Reaction, Zn(s) + Cu2+(aq)…

Q: The value of Kyg for AgBr is 5.4 x 1013. For the Ag/AgBr electrode, AgBr(s) + e Agls) + Br'(aq)…

Q: What is the calculated value of the cell potential at 298K for an electrochemical cell with the…

Q: A voltaic cell is made using the two half-cells below (both written as reduction): Cl2(g) + 2e¯ 5…

A: The cell in which chemical energy is converted into electrical energy is called Galvanic cell…

Q: 4) The Zn/Cu battery operates using the following redox reactions: + 2e → Cu) E° = 0.34V Cua Zn + 2e…

A: Zn2+(aq) + 2e- -> Zn(s) Eo = -0.76 Cu2+(aq) + 2e- -> Cu(s) Eo = 0.34…

Q: A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a…

A: The objective of the question is to write the balanced equation for the overall reaction in acidic…

Q: A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is…

A: The call reaction at anode is, H2(g) ------> 2H+(aq) + 2e- Standerd cell potential of the cell =…

Q: Question 11 Calculate the cell potential at 25°C for the Cris)|Cr3"(aq)||Sn"(aq)|Sn(s)…

A: 11) Given, Cell notation: Cr(s)|Cr3+(aq)||Sn2+(aq)|Sn(s) [Cr3+] = 1.50 M [Sn2+] = 0.090 M Cell…

Q: The following electrochemical cell is constructed at standard state: Mg(s) | Mg2+ || Cr2+ | Cr(s) a)…

A: Answers are explained below.

Q: What galvanic cell can be constructed to yield the most positive standard cell potential using the…

A: We have given that Standard reduction potential E°red Cu2+ + 2e- → Cu +0.34V…

Q: X(s)|X3+ (2.04 M) || Mn O4 1 minus (1.62 M)|Mn2+ (0.25 M)|H+ (2.64 M) The reduction potential for…

A: Given The concentration of X3+ is 2.04 M. The concentration of MnO4- is 1.62 M. The concentration…

Q: Some Na2S is added to the Pb2+ compartment, precipitating some Pb2+ as lead sulfide. ___The…

Q: XX (0.80 M) || Mn O4minus (1.96 MIMn (2.35 MH" (1.52 M) The reduction potential for X is 1.17 V. The…

Q: The value of K, for AgBr is 5.4 x 1013. For the Ag/AgBr electrode, AgBr(s) + e Ag(s) + Br°(aq)…

A: Given, Reaction : AgBr(s)+e-→Ag(s) +Br-(aq) E°=0.070 V The Ksp value 5.4×10-13

Q: A Zn-Ag Galvanic cell has an Ecell value of 1.536 V. The cell diagram is as blow. Calculate the…

A: This is a simple question of electrochemistry for the application of Nernst equation.

Q: A student is given two beakers in the laboratory. One beaker contains a solution that is 0.14 M in…

A: Given: [Mn3+ ] = 0.14 M [Mn2+ ] = 0.46 M [Sn2+ ] = 0.28 M And [Sn4+ ] = 0.056 M

Q: An electrolytic cel besed on the reaction represented above wes constructed from zinc and copper…

A: Given that : Standard cell potential = 1.10 V Observed cell potential = 1.00 V We need to determine…

Q: Determine the cell potential and the equilibrium concentrations of the following concentration cell:…

A: The given cell notation is: Cu|Cu2+0.020 M||Cu2+2.0 M|Cu It is a concentration cell (electrolytic…

Q: Determine the voltage of a galvanic cell composed of Ba(s) in a 1.00 M solution of Ba²+, and Sn(s)…

A: Answer:-This question is answered by using the simple concept of calculation of standard cell…

Q: a) How many grams of Nickel (58.6934 g/mol) can be plated on to an iron base metal if 200.0 Amps of…

A: Electrolyte is a material which if dissolved into a polar solvent, generates an electrically…

Q: he reaction Ni+Cl2→Ni^(+2)+2Cl^- has an overall cell potential equivalent to 1.59 V. Is the reaction…

A: Given : We have to predict whether the reaction is spontaneous or non spontaneous.

Q: voltaic cell employs the redox reaction: Au(s) + 3 Na+(aq) → 3 Na(s) + Au3+(aq) E°cell = -4.21 V…

A: The solution is as follows:

Q: Study each overall cell reaction. Identify and write the half-reaction that occurs in the an the…

A: Given : We have to tell whether the reaction is spontaneous or not.

Q: An electrochemical cell consists of a standard hydrogen electrode and a copper metal electrode. a.…

A: #(a): Since Cu(s) is less reactive than hydrogen, Cu2+(aq) will be reduced and H2(g) will be…

Q: A silver wire coated with AgCl is sensitive to the presence of chloride ion because of the half-cell…

A: Concentration of CuSO4 solution = 1 (M) Measured cell potential = 0.0518 V

Q: Hi! I am having trouble with this. I used the nernst equation and got concentration = 0.5467 but am…

Q: X(s)|X4+ (0.87 M) || Mn O4 1 minus (1.61 M)|Mn2+ (2.98 M)|H+ (1.49 M) The reduction potential for…

A: Given information: Reduction potential for X4+ = 2.22 V Reduction potential for MnO4- = 1.51 V

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

A: The given redox reaction is, MnO2(s)+4H+(aq)+2Cr2+(aq)→Mn2+(aq)+2H2O(l)+2Cr3+(aq) The overall…

Q: X(s)|X4+ (2.75 M) || Mn O4 1 minus (2.58 M)|Mn2+ (2.75 M)|H+ (0.30 M) The reduction potential for…

A: According to the cell diagram given,Anode is at left side to salt bridge and cathode is at right…

Q: X(s)|X3+ (1.14 M) || Mn O4 1 minus (1.97 M)|Mn2+ (0.64 M)|H+ (2.79 M) The reduction potential for…

A: Given data,EoX3+/X=0.46VEoMnO4-/Mn2+=1.51VX(s)|X3+ (1.14 M) || MnO4- (1.97 M)|Mn2+(0.64 M)|H+ (2.79…

Q: Given the following standard reduction potentials: Ag, Eº=0.80 V Ag+ + e Cu²+ + 2e Cu, Eº=0.34 V…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: Calculate the standard cell potential for this reaction.

A: Here, we have to find the standard cell potential for the given reaction using the standard…

Q: Hydrogen bromide dissociates into its gaseous elements, H₂ and Br2, at elevated temperatures. HBr(g)…

Q: Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an…

A: In certain reactions, transfer of electrons takes place from one species to another. There are two…

Q: Calculate the theoretical potential of the following cells. Indicate whether the reaction will occur…

Q: Consider a galvanic cell below and calculate the concentration of Au*3 solution. The measured cell…

Q: Consider the following cell reaction: Zn(s) + 2 H*(? M) —>Zn²+ (1.00 M) + H2(g)(1.00 atm) If the…

A: Answer:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: Calculate the value of the EMF of galvanic cells and write the electrode reactions occurring in…

A: a) Zn/Zn2+(0.001)∥Cd2+(0.1)/Cd Anode : Zn = Zn2+ + 2e-…

Q: Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an…

A: Redox reaction is a reaction which involves transfer of electrons from one species to another…

Q: X(s)|X3+ (1.14 M) || Mn O4 1 minus (1.97 M)|Mn2+ (0.64 M)|H+ (2.79 M) The reduction potential for…

A: Pt(s) || Sn2+ (0.0032 M),Sn4+(0.10 M) ‖ Fe3+(0.12 M),Fe2+(0.0053 M) || Pt.(s) Oxidation at anode :…

Q: Determine emf of the cell: Fe(s) | Fe(NO3)3 (0.015M) || Zn(NO3)2 (0.025 M) | Zn(s)

Q: A voltaic cell represented by the following cell diagram has Eell =1.280 V. Za(s)|Zn (1.00 M)||Ag*…

Q: One electrode in an alkaline battery is zinc, and the other is manganese dioxide. (a) Fill in the…

A: Alkaline battery is a primary battery which extracts energy from the reaction between zinc and…

Q: 30) Write the balanced overall reaction and calculate the standard cell emf (E) for: Al(s) | Al"(aq)…

Q: 9) The standard cell potential (E°cell) for the voltaic cell based on the reaction below is_ 3Fe2+…

A: The objective of the question is to calculate the standard cell potential (E°cell) for the given…

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

A voltaic cell consists of Co I Co?²*(0.25 M) II Cu²*(0.35M) I Cu. The electrode potential
at this concentration is [A] 0.6157V [B] 0.6025 V [c]0.6243V [D] 0.5014 V
(Co* + 2 e→ Co, ɛ°red = -0.28 V, Cu²* +2 e→ Cu, ɛ°red = +0.34 V)
A
C
O D

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

For a standard voltaic cell comprised of a Cu2+|Cu electrode and a Fe2+|Fe electrode, what is the cell potential, in volts?
4. The cell diagram for an electrochemical cell is given below: Mn(s) | Mn* (aq, 1.0 mol dm) || Ag* (aq, 1.0 mol dm)|Ag (s) In the above cell, the standard electrode potential of the silver hal f-cell is =0.80 V. E°cell = +1.98 V Write the equation for the reaction occurring at the anode and cathode. Write the overall cell equation Determine the standard electrode potential of the Mn2*/Mn half-cell What is the strongest oxidizing agent in the above cell? What is the strongest reducing agent in the above cell? a) 1) ii) b) i) i1) c) After the cell was used, the change in mass of the silver electrode was found to be 5.40 IS g Caleulate the change in mass of the manganese electrode.
5) In an electrochemical cell, Cue is placed in the anode half-cell while Age in the cathode half-cell. The standard potential of the half-reactions are as follows: Ag* (ag)+ e¯→ Ag(s) E°red = +0.80 V Cu²+, (aq) + 2 е — Сu(g) E°red = +0.34 V a) What is the standard potential of the cell, E°ell? b) Is the reaction spontaneous or non-spontaneous?
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (PH, )= latm) immersed in a solution of unknown [H*]. If the cell potential is 0.216 V, what is the pH of the unknown solution at 298 K? pH =
Consider the following cell reaction: Fe(s) + 2 H"(? М) —Ғе*"(1.00 М) + H-(g)(1.00 atm) →Fe? If the cell potential at 298 K is 0.164 volts, what is the pH of the hydrogen electrode? pH
The potential of the following voltaic cell is 0.55 V. Given this information, determinethe Kb for the organic base (RNH2) dissolved in the left cell.
Question 4: (a) What are redox reactions? Explain the difference between a gal- vanic and an electrolytic cell. Consider the cell described below: Al | AP"(1.00M) | Pb³"(1.00M) | Pb Calculate the cell potential after the reaction has operated long enough for the [Al"] to have changed by 0.60 mol/L. (Assume T = 25°C.) (b) Many elements have been synthesized by bombarding relatively heavy atoms with high-energy particles in particle accelerators. Complete the fol- lowing nuclear equations, which have been used to synthesize elements. U + C-→ Cf + Cf + 'B Lr + + He Bk + in + 6 n 10 Db + 4 in 103
Please explain, answer 0.57 V
The cell potential was 1.271 V at 25oC and a Al3+(aq) concentration of 0.178 M. What was the hydronium ion concentration? The H2(g) pressure was 1 atm at 25oC.6H+(aq) + 2Al(s) ↔ 2Al3+(aq) + 3H2(g) Ecoell = 1.660 V
Ex 12. If a galvanic cell consists of cadmium and lead electrodes immersed in monomolar solutions of their soluble salts, the TRUE statement is: (a) the mass of the Pb electrode decreases and the mass of the Cd electrode increases; (b) electrons pass from the lead to the cadmium electrode; (c) oxidation is performed on the Cd electrode; (d) the electromotive voltage remains constant during operation of the element ºcd²+/cd= -0,403 V; ºpb²+/Pb = -0,126 V Justify your answer!
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ( PH, )= latm) immersed in a solution of unknown [H*]. If the cell potential is 0.201 V, what is the pH of the unknown solution at 298 K? pH =
9:-0 electrode is called (a) anode, oxidation (b) anode, reduction O (c) cathode, oxidation (d) cathode, reduction (e) cannot tell unless we know the species being oxidized and reduced. The standard electrode potentials of the electrodes Cu+ | Cu and Ag+ | Ag are 0.337 V and 0.7991 V. What would be the concentration of Ag+ in a solution containing 0.06 M of Cu*+ ion such that both the metals can be deposited together. Assume that activity coefficients are unity and both silver and copper do not dissolve among themselves. 12.98x10-8 mole/dm-3 15.22x10-8 mole/dm-3 10.37x10-8 mole/dm-3 The standard electrode potentials of the electrodes Ag+ | Ag and Fe+, Fe* | Pt are 0.7991 V and 0.771 V respectively. Calculate the equilibrium constant for the reaction