A voltaic cell using Pb2+/Pb and Ni²+/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 21.0 hours at 25.0°C? (E° for Pb2+/Pb = -0.130 V and E° for Ni2+/Ni = -0.250 V.)

A voltaic cell using Pb2+/Pb and Ni²+/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 21.0 hours at 25.0°C? (E° for Pb2+/Pb = -0.130 V and E° for Ni2+/Ni = -0.250 V.)

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 these two entries from a fictional table of standard reduction potentials. X³+ + 3 e y³+ +…

Q: Write the equation for the cell reaction and calculate the standard emf of a cell that uses Mg/Mg2+…

Q: Consider the electrolysis reactions cathode Cu?"(aq, 0.177 M) + 2e-= Cu(s) H,O) =0,(g, 1 bar) + 2H*…

Q: What is the pH of the solution in the cathode half-cell when PH2 = 1.0 atm, 3Zn2+4 in the anode…

A: The anodic half-reaction and cathodic half-reaction that occurred in the electrochemical cell are as…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

Q: Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd2+ + 2 e Cd (a)…

Q: • Part D Hg (1) + HgCl, (aq) → Hg,Cl2 (s) Express your answer using ftwo significant figures. ΑΣφ ?…

A: The given reaction, Hg(l)+HgCl2(aq) → Hg2Cl2(s)

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: What will be the overall balanced reaction if you want to make a galvanic cell? What is the…

Q: When [Hg2+] = 1.37 M, the observed cell potential at 298 K for an electrochemical cell with the…

Q: A voltaic cell using Pb²+/Pb and Ni²+/Ni half-cells is set up at standard conditions, and each…

A: Here we have to determine the Ecell of the following given standard galvanic cell after passing 0.15…

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: The galvanic cell contains two half-cells: Ni/Ni2+ and Co/Co2+. Initial concentrations: [Ni2+] =…

Q: How long will an electrolytic cell containing a solution of cadmium(II) iodide need to run at a…

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 galvanic cell is constructed using two half-cells in standard state: Al|Al3+ and Ni|Ni+2 Al3+(aq)…

A: To find out the standard cell potential, first check out which species are oxidized and reduced.…

Q: When [Pb+1=1.01 M, the observed cell potential at 298 K for an electrochemical cell with the…

Q: A galvanic cell is made of a Ni2+/Ni half cell with [Ni²*] = 6.00 × 10-² M and an Ag*/Ag hal cell…

Q: Given the following two half-reactions, write the overall reaction in the direction in which it is…

A: Given two half cell reactions are : Options are : a). Overall cell reactions = ? b). Standard cell…

Q: Use the References to access important values if needed for this question. Use standard reduction…

A: " Since you have posted multiple questions, we will provide the solution only to the first question…

Q: What is the overall cell reaction of a galvanic cell employing the following half-reactions? NiO2…

A: Given : half cell reaction Tip : cell having higher value of reduction potential will reduced

Q: A galvanic cell is constructed using the following two half-cells at 25°C and 1 atm. The…

A: Answer:- This question is answered by using the simple concept of electrochemistry which involves…

Q: A certain half-reaction has a standard reduction potential Ed=-0.06 V. An engineer proposes using…

Q: (iv) Calculate the cell voltage for the reaction.

A: We have to find cell voltage. So, we will you "(Nermest equation)". Which is Ecell =…

Q: 0.10 М MnOg 0.40 М Cr3+ 0.20 М Mn2* 0.30 М Cr,0,2- 0.010 МН" 0.010 МН'

A: Given data: Eocell for Mn = 1.52 V Eocell for Cr = 1.33 V Formula used: Q=[products][reactants]

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

A: Given Ecell =0.189we know E°cell is 0 for hydrogen cell.

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e X(s)…

A: E° cell = E° cathode + E° anode At anode always oxidation occur At cathode always reduction occur…

Q: A. H2O2 (aq) + Cl2 (g) B. acidified H2O2+ MnO2 (s) C. NaCl (aq) + acidified H2O2 (aq D. NaCl (ag) +…

A: Correct Answer is (D) where there is no effervescence of gas. In (A), (B) and (C), all case there…

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

A: Given-> E°Ni2+/Ni = -0.25 V E°Co2+/Co = -0.28 V

Q: The voltaic cell described by the notation below measured a potential of 1.1 V. If the reaction was…

A: The given cell notation for the voltaic cell is:- Pt(s) | J2- (1.50 M) | J(l) || Ag+ (0.010 M) |…

Q: standard cell potential f

Q: 2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →…

A: The objective of the question is to find the concentration of H+ ions, the pH of the cathodic…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: We have to predict the reaction at cathode , anode and overall cell reaction , also we have to…

Q: Consider the following two half-reactions and their standard reduction potentials for a voltaic ce…

A: Electrode for which the value of reduction potential is higher has higher chances of being reduced.…

Q: A galvanic cell is set up using the redox reaction below at 298 K. If the cell has a standard cell…

A: Since the value of ΔG0 is given by ΔG0 = -nFE where E = standard cell potential = 0.31 F =…

Q: A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each…

A: The cell potential after it has delivered 0.150 A for 11.0 hours at 25°C is to be calculated.

Q: Consider a galvanic electrochemical cell constructed using Cr/Cr** and Zn/Zn2* at 25 °C. The…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: The emf of a standard X-Y galvanic cell is -2.763V. If the standard half-cell emf for the oxidation…

A: The overall cell reaction is the sum of the two half-reactions, but the cell potential is the…

Q: Consider a Galvanic cell constructed from the following half cells, linked by an external circuit…

Q: A voltaic cell is constructed that uses the following reaction and operates at 298 K. (a) What is…

Q: A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential…

A: In an electrochemical cell, the reduction of the chemical species takes place that is having the…

Q: Use the standard half-cell potentials listed below to calculate the standard cell potential for the…

A: Given: K+(aq) + e- → K(s), E∘ = -2.93 V I2(s) + 2e- → 2I-(aq), E∘ = +0.54 V We have to find…

Q: Use the data in Appendix D in the textbook to calculate the standard cell potential for each of the…

Q: Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3e- X(s)…

A: The solution is as follows :

Q: epared according to the redox reaction shown below. A voltmeter connected to this galvanic cell…

A: Ecell = 0.45V

Q: A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations:…

Q: A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard…

A: Oxidation - It is the removal of an electron from an atom or ion. It takes place at the anode…

Question

100%

A voltaic cell using Pb2+/Pb and Ni2+/Ni half-cells is set up at
standard conditions, and each compartment has a volume of
355 mL. What is the cell potential, in V, after it has delivered
0.150 A for 21.0 hours at 25.0°C? (E° for Pb2+/Pb = -0.130 V
and E° for Ni2+/Ni = -0.250 V.)

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: Defining volatic cell!

VIEW

Step 2: Finding out the charge that is passed through the solution!

VIEW

Step 3: Finding out the initial moles of each ion!

VIEW

Step 4: Finding out the moles of nickel ion after the current passed!

VIEW

Step 5: Finding out the moles of lead ion after the current passed!

VIEW

Step 6: Finding out the value of standard cell potential!

VIEW

Step 7: Finding out the value of cell potential!

VIEW

Solution

VIEW

Step by step

Solved in 8 steps with 19 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

2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →Zn²+ze E = 0.76 V If the voltage of the cell is 0.45V at 25°C when [Zn²] = 1.0 M and PH₂ = 1.0 atm, what is [H+]? 2H+ + 2e- → H₂ EⓇ = 0.0V (b) For the voltaic cell described in part (a), find the pH of the cathodic solution when pH2 = 1.0 atm and [Zn²+]= 0.1 M and the E*cell = 0.542 V. (c) What amount of time is needed to plate 2.08 g of copper at a constant current flow of 1.26 A from a 0.1 M CUSO4 solution? Cu²+ +ze--- Cu(s)
Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following half-cell systems: Ag+(0.010M) + e- --> Ag Eo= +0.80 V Cr3+(O.010M) + 3e- --> Cr Eo= -0.74 V
A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)
A galvanic cell consists of a Ni/Ni²+ half-cell and a Co/Co²+ half-cell with initial concentrations: [Ni²+] = 0.80M and [Co²+] = 0.20 M at 298.15 K. half-reaction Eº (V) Ni²+ (aq) +2e→Ni(s) -0.25 Co²+ (aq) +2e→Co(s) -0.28
MnO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify the oxidizing agent and anode. C) standard cell potential? D) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
(ii) State which species is the oxidising agent.
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative
(c) A galvanic cell is constructed using the following two half-cells at 25°C and 1 atm. The concentration of each species is given in the half-cell equation. Fe* (aq, 1.10 mol dm³) +3e → Fe2+ (aq, 0.86 mol dm³) E° = +0.77 V Ag* (aq, 1.35 mol dm³) + e → Ag(s) E° = +0.88 V
Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V
A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25.0 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)
Consider the half reactions in a cell: Pb2+ + 2 e ------ Pb(s) Eo = - 0.126 V Fe3+ + e ------ Fe2+ (aq) Eo = + 0.771 V Which of the following statement is correct for the cell? Given Given A. For a Galvanic cell the standard emf will be 0.645 V and Pb will be the anode B. For a Galvanic cell standard emf will be 0.645 V and Fe will be the cathode C. For a Galvanic cell standard emf will be 1.668 V and Pb will be cathode D. For a Voltaic cell the standard emf will be 0.897 V and Fe will be the anode E. For a Voltaic cell standard emf will be 0.897 V and Pb will be the anode