55) What is the concentration of Cu2+ in the following cell at 25°C if the cell voltage is ¹253 V? 0,952 V Zn Zn2+ (0.125 M) | Cu2+(?) | Cu Cu2+ +2 e-→ Cu(s) E° = 0.340 V Zn2++2 e-→ Zn(s) E°= -0.763 V A) 9 × 10-4 M B) 0.6 M C) 1 x 10-2 M D) 1 x 10-6 M E) 4 x 10-4 M

55) What is the concentration of Cu2+ in the following cell at 25°C if the cell voltage is ¹253 V? 0,952 V Zn Zn2+ (0.125 M) | Cu2+(?) | Cu Cu2+ +2 e-→ Cu(s) E° = 0.340 V Zn2++2 e-→ Zn(s) E°= -0.763 V A) 9 × 10-4 M B) 0.6 M C) 1 x 10-2 M D) 1 x 10-6 M E) 4 x 10-4 M

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: For the galvanic (voltaic) cell: Zn(s) + 2TI*(aq)→ 2TI(s) + Zn2* (aq) E cell = 0.42 V If the…

Q: When the Cu2+ concentration is 1.16 M, the observed cell potential at 298K for an electrochemical…

A: In the given cell, copper is undergoing reduction at anode and aluminium is getting oxidized at…

Q: 5) In an electrochemical cell, Cu9) is placed in the anode half-cell while Ag) in the cathode half-…

Q: • Part A Identity the coefficients in the reaction Enter your answers in order from left to right…

A: Given reaction1 reaction 2

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

A: 3Cu2+ (aq) + 2Al (s) -----> 3Cu (s) + 2Al3+ (aq) [Cu2+] = 7.62 M [Al3+] = 3.54 M

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

A: We have two half cell reaction: X3+ + 3e- ----> X(s) E°= -1.61 V Y3+ + 3e- ---->…

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: O ELECTROCHEMISTRY Designing a galvanic cell from two half-reactions OODV3 A chemist designs a…

A: Since you have asked a question with multiple sub-parts, as per our company guidelines we are…

Q: What is the voltage of the half cell AgCl (s) + e- ↔↔ Ag (s) + Cl- (aq) with the concentration of…

A: Given data - half cell - AgCl (s) + e- ↔↔ Ag (s) + Cl- (aq) concentration of KCl = 1.0 M Eo= 0.222…

Q: Question 7 Which of the following cells is most likely to be an example of a galvanic cell? A) Zn(s)…

A: Answer:-This question is answered by using the simple concept of Galvanic cell which is also called…

Q: Calculate the potential of the electrochemical cell and determine if it is spontaneous as written at…

A: Given that, an electrochemical cell is Cus|Cu2+0.11 M||Fe2+0.0063 M|Fes. Also, the standard…

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

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: What is E°(cell) for the cell Mn | Mn²⁺(aq) || Ag⁺(aq) | Ag? Standard Reduction Potential: Au³⁺(aq…

A: Thank you.

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

Q: Consider the redox reaction Ag*(aq) + Cu(s) ► Ag(s) + Cu²*(aq) Calculate the E'cell and state if the…

A: Given reaction: Ag+(aq) + Cu(s) ----->> Ag(s) + Cu2+(aq) Gibbs free energy: Gibbs free energy…

Q: O ELECTROCHEMISTRY Understanding concentration cells 1/5 A certain metal M forms a soluble sulfate…

Q: 7. A galvanic cell at 25°C consists of an electrode of zinc in a 0.10 M ZNSO4 solution and anther of…

A: An electrochemical cell is a type of cell which converts chemical energy into electrical energy.…

Q: The voltage generated by the zinc concentration cell described by the line notation Zn(s) Zn²+ (aq,…

A: The cell given isZn(s) | Zn2+ (aq,0.100 M) ‖ Zn2+ (aq,? M) | Zn(s)Since in any cell, the first half…

Q: When the Cu²+ concentration is 1.07 M, the observed cell potential at 298 K for an electrochemical…

A: To determine the concentration of product, we will follow the following steps: 1) determine E°cell…

Q: Determine the cell potential for an electrochemical cell (not standard condition, E) based on…

A: GIVEN: Reactions: To Solve: Cell potential for an electrochemical cell=?

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: Consider electrode potential data given in the picture Predict which two electrodes combination will…

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: Calculate the theoretical cell potential for the following galvanic cell: Zn | Zn2+…

A: Theoretical cell potential can be calculated by using Nernst Equation. Cell notation and standard…

Q: When the Cu²+ concentration is 1.26 M, the observed cell potential at 298 K for an electrochemical…

A: Multiple questions

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: half-reaction standard reduction potential MnO,(aq)+2H,0(1)+3e MnO,(s)+4 OH (aq) E=+0.59 V red 2+…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

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: Given the standard electrode reduction potentials, which reaction will occur spontaneously? Standard…

A: Given: Half-cell reactions: Cu+2 (aq) + e- → Cu+ (aq) Eo = +0.15 V V+2 (aq) + 2e- → V (s)…

Q: Calculate AG for the electrochemical cell Pb(s) | Pb 2(aq) || Fe (aq) | Fe 2(aq) | Pt(s) A) -1.2 x…

A: Answer:Here:n is equal to number of electrons transferred from anode to cathode in balanced cell…

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

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: The voltage generated by the zinc concentration cell described by the line notation Zn(s) ∣∣…

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

A: The solution is as follows :

Q: The voltage generated by the zinc concentration cell described by the line notation Zn(s) | Zn²…

Q: The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V.…

A: Ecell = Eocell - 0.0591/n log[product]/[reactant]

Q: Zn2+ taking place at the anode? Consider the cell Zn || Cu²+ Cu . What half reaction is Zn(s) → Zn²+…

A: Given cell is, Zn | Zn 2+ || Cu2+ | Cu

Q: A chemist designs a galvanic cell from the following two half-reactions NO3(aq) + 4H+ (aq) + 3e →…

A: Given that, for a galvanic cell, two half-cell reactions are NO3-aq + 4H+aq + 3e- → NOg + 2H2Ol…

Q: Consider the following half-reactions: E° = +2.87 V F2(9) + 2 e ® 2 F'(aq) Cu2*(aq) + 2 e¯ ® Cu(s)…

A: To reduce Al+3 to Al the compound used must have more negative reduction potential than Al+3.

Q: For the following reaction, predict the measured cell potential (Ecell) if the pressure of O₂ is…

Q: ›Calculate the cell potential for the galvanic cell in which the given reaction occurs at 25 °C,…

Question

55) What is the concentration of Cu2+ in the following cell at 25°C if the cell voltage is ¹253 V?
0,952 V
Zn Zn2+ (0.125 M) | Cu2+(?) | Cu
Cu2+ +2 e-→ Cu(s) E° = 0.340 V
Zn2++2 e-→ Zn(s) E°= -0.763 V
A) 9 × 10-4 M
B) 0.6 M
C) 1 x 10-2 M
D) 1 x 10-6 M
E) 4 x 10-4 M

AI-Generated Solution

AI-generated content may present inaccurate or offensive content that does not represent bartleby’s views.

Unlock instant AI solutions

Tap the button
to generate a solution

Click the button to generate
a solution

SEE SOLUTION

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)
The free energy change for the following reaction at 25 °C, when [Sn2+] = 1.19 M and [Zn2+] = 7.83×10-3 M, is -133 kJ: Sn2+(1.19 M) + Zn(s)→ Sn(s) + Zn2+(7.83×10-3 M) AG = -133 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
The redox reaction 3 Cl, (g) + 2 Al(s) → 2 Al³ † (aq) + 6 CI"(aq) consists of the two half-reactions shown. Cl, (g) + 2 e- –→ 2 Cl¯(aq) E. red = +1.36 V Al3 + (aq) + 3 e Al(s) Eed = -1.66 V What is the standard cell potential? 3.02 V 7.70 V -3.02 V O -0.30 V
7
Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00 M solution of A certain metal M forms a soluble sulfate salt M₂ M₂(SO4)3 and the right half cell with a 2.50 mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 left right × S
q19
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?
Standard Electrode Potentials at 25 °C Reduction Half-Reaction O Cu (aq) O H,Ozlaq) O Br O 10₂ (aq) Fyl) +20 H₂O₂(aq) + 2 H(aq) +2e" PbOg(s) +4 H(aq) +50, (aq) + 2 e Mn0 (aq) +4 H(aq) + 3 e MnO, (aq) +8H(aq) + 5 e Au³(aq) + 3 e PbOy(s) +4 H(aq) + 2e¯ C+20 00, (aq) +14 H(aq) + 6 e 00+ 4H*(aq) + 4 MnO₂ (s) +4 H(aq) +2e¯ 10₂(aq) + 6H(aq) +5e Big(0+20 VO₂ (aq) + 2 H(aq) + e¯ NO₂ (aq) + 4H(aq) + 3 e CO₂(0)+ Ag (ag)+e Fe(aq) + e 0)+2 H(aq) +2 e Mn0, (aq) + e (8) +26 Cu (aq) + e -2 (aq) -2 H₂O(0) Which of the following is the strongest oxidizing agent? -PbSO4(s) + 2 H₂O(0) →→MnO₂ (s) + 2 H₂O(0) Mn²(aq) + 4H₂O(1) - Au(s) ·Pb²+ (aq) + 2 H₂O(0) - 2 Cr (aq) 2 Cr³+ (aq) + 7 H₂O(1) → 2 H₂O( -2(aq) -Cu(s) Mn²+ (aq) + 2 H₂O(0) ₂(aq) + 3 H₂0(0) -2 Br (aq) - Vo²+ (aq) + H₂O( -NO(g) + 2 H₂O(1) — CIO; (aq) -Ag(s) -Fe²+ (aq) -) HyOz(ag) MnO₂ (aq) 1.00 0.96 0.95 0.80 0.77 0.70 0.56 0.54 0.52 E° (V) 2.87 1.78 1.69 1.68 1.51 1.50 1.46 1.36 1.33 1.23 1.21 1.20 1.09
(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
A voltaic cell is constructed with two silver electrodes, where the half-reaction isAg2+(aq) + 2e- → Ag (s) E° = -0.322 VDetermine the cell emf at 25 °C when the concentrations of chloride ion in the two compartments are 4.0 Mand 0.050 M, respectively.
Calculate the theoretical cell potential for the following galvanic cell: Mg | Mg2+ ( 1 M) || Cu2+ (2 M) | Cu
3. What is the E'c for the cell represented by the combination of the following half-reactions? 2Hg**(aq) + 2e = Hg,"(aq); E= 0.92 V Cr* (aq) + 3e - Cr(s), E"= -0.74 V