In a certain zinc-copper cell, Zn(s) + Cu2+(aq) – Zn2*(aq) + Cu(s) the ion concentrations are [Cu2*] = 0.0234 M and [Zn2+] = 1.8 M. What is the cell potential at 25 °C? Ecell = i V

In a certain zinc-copper cell, Zn(s) + Cu2+(aq) – Zn2(aq) + Cu(s) the ion concentrations are [Cu2] = 0.0234 M and [Zn2+] = 1.8 M. What is the cell potential at 25 °C? Ecell = i 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: In a certain zinc-copper cell, Zn(s) + Cu2*(aq) –→ Zn²*(aq) + Cu(s) the ion concentrations are…

A: Given equation : Zn(s) + Cu2+ (aq) -------> Zn2+ + Cu(s) [Cu2+] = 0.0195M [Zn2+] = 1.4M Ecell =…

Q: Calculate the cell potential of a cell operating with the following reaction at 25°C in which…

Q: An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* 1.0 M…

A: A numerical problem based on Nernst equation, which is to be accomplished.

Q: andard potentials given in the appendices s for the following reactions: Cu(s) +2Ag*(aq) Cu2*…

A: In an electrochemical cell, the standard cell potential can be calculated by using the following…

Q: What is K for the reaction Zn(s) + Cu²*(aq) ® Zn²*(aq) + Cu(s), given E°cell is 1.1 V at 25 °C for…

Q: The standard cell potential for the reaction: A (s) + B2* (aq) = A2* (aq) + B (s) is - 0.371 V. What…

Q: Calculate the cell potential for a cell at 39oC with a Cu2+ concentration of 0.02 M and a Zn2+…

A: The given data contains, Concentration of Cu2+= 0.02 M Concentration of Zn2+=0.066 MEcell0 =1.10 V…

Q: For the reaction 2C03+ (aq) + 2CI- (aq)→2C0²+(aq) + Cl2 (g). E° =0.483 V what is the cell potential…

A: Cell potential is calculated using Nernst equation .

Q: Part A For the reaction 2Co (aq) + 2Cl(aq)→2Co² (aq) + Cl₂(g). E=0.483 V what is the cell potential…

Q: For the reaction 2Co+ (aq) + 2Cl (aq)→2C02+ (aq) + Cl2 (g). what is the cell potential at.25°C if…

A: Given that, a cell reaction is 2Co3+(aq) + 2Cl-(aq) →2Co2+(aq) + Cl2(g). The concentrations are…

Q: The measured cell potential, Ecell, for the cell shown is -0.3645 V at 25 °C. Calculate the H*…

Q: Calculate the cell potential for the galvanic cell in w

Q: Calculate the non-standard cell potential (in V) for the following reaction at 190.51 ℃ with the…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 33.56 ℃ with the…

A: The cell reaction taking place is given as, => Pb2+ (aq) + Li (s) ------> Pb (s) + Li+ (aq)…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 178.7℃ with the…

Q: Calculate the cell potential for the galvanic cell in which the reaction Ti(s) + Co² (aq) Ti² (aq) +…

A: Cell potential of any complete cell can be measured by Nernst equation. This question will be solved…

Q: Given that the standard electrode potentials (E°) of metals are:K+/K = -2.93 V, Ag+/Ag = 0.80…

A: standard electrode potentials (E°) is inversely proportional to reducing power Higher standard…

Q: The cell potential for this reaction is, V when [ Zn2*] = 1.0 M and [Pb2*] = 2.0 x 10-4 M. Pb2+ (aq)…

A: The cell potential is calculated by Nernst equation . E = E° - (0.0591/n) log Qc E = cell potential…

Q: Calculate ΔG° for the electrochemical cell Pb(s) | Pb ⁺²(aq) || Fe ⁺³(aq) | Fe ⁺²(aq) | Pt(s) A)…

Q: Zn(s) + Cu²+ (aq) → Zn²+ (aq) + Cu(s) the ion concentrations are [Cu²+] = 0.0389 M and [Zn²+] = 1.7…

Q: Calculate the cell potential for the galvanic cell in which the reaction Cd(s)+Cu2+(aq) ⁢->…

Q: The standard cell potential for the reaction at 298.15 K: Fe (s) + Zn2+ (aq) ⇋ Fe2+ (aq) + Zn (s)…

Q: Calculate the cell potential for a cell at 42oC with a Cu2+ concentration of 0.008 M and a Zn2+…

Q: Calculate the cell potential for the galvanic cell in which the reaction Fe(s) + Au*(aq) =…

A: The question is based on the concept of electrochemistry. the electrode which has higher reduction…

Q: For the reaction 2Co 3+(aq)+2Cl -(aq)→2Co 2+(aq)+Cl 2(g) E∘=0.483 V what is the cell…

A: P ( Cl2 ) = 4.10 atm P V = n R T P = ( n/ V ) R T = c R T c = P / R T T ( temperature ) = 25…

Q: 1) The standard reduction potentials of Cu2+ (aq) Cu(s) and Ag+ (aq) Ag(s) are +0.34 and +0.80 V,…

A: Calculate the cell potential of the given galvanic cell. Given At Anode Cu/Cu2+; E°=-0.34 V At…

Q: Calculate the cell potential for a cell at 29oC with a Cu2+ concentration of 0.017 M and a Zn2+…

A: Oxidation is lose of electrons. Reduction is gaining of electrons.

Q: The standard cell potential for reaction, Fe(s) + Cu²⁺(aq) → Fe²⁺(aq) + Cu(s) is E⁰ = 0.17V. What is…

A: The cell reaction given is, => Fe (s) + Cu2+ (aq) -------> Fe2+ (aq) + Cu (s) Given : Standard…

Q: In a certain zinc–copper cell, Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) the ion concentrations are [Cu2+]…

Q: Which of the following cells is most likely to be an example of a galvanic cell? Zn(s) | Zn2+ ||…

Q: 16) Using these metal ion/metal standard reduction potentials: Fe2+ (aq) Fe(s) Zn²+ (aq)|Zn(s) -0.44…

A: We know Oxidation occurs at anode and reduction occurs at cathode . Cell potential is an intensive…

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

A: [Cr2+] = 0.00190 M [Au3+] = 0.824 M ->Answer may differ slightly because values of standard…

Q: Calculate the cell potential for the galvanic cell in which the reaction Al(s)+Au3+(aq)↽−−⇀…

Q: Calculate the non-standard cell potential (in V) for the following reaction at 65.86 ℃ with the…

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

Q: where the half-cells are Ag|AgNO3(aq) and Ni|Ni(NO3)2(aq), and the electrode potentials are as…

A: Standard cell potential (Eo) is the EMF of the cell when the concentrations of electrolytes is 1M ,…

Q: Calculate the cell potential of tho following cell at 25°C. Cr(s) | C" (1.0 X 10° M) || Ni²* (1.5 M)…

A: Given data,[Cr3+]=1.0×10-3M[Ni2+]=1.5MTemperature=25oC

Q: Calculate the cell potential for a cell at 30°C with a Cu2+ concentration of 0.012 M and a Zn²+…

Q: A reaction 1 Ag*(aq) + H2 (g) → H* (aq) + Ag(s) Takes place in a cell and the standard cell…

A: Ag+ (aq) + 0.5 H2 (g) ==> H+(aq) + Ag(s)

Q: The standard cell potential for the reaction at 298.15 K: Fe (s) + Zn2+ (aq) ⇋ Fe2+ (aq) + Zn (s)…

Q: The cell reaction NiO₂ (s) + 4H+ (aq) + 2Ag(s)- Ni²+ (aq) + 2H₂O + 2Ag+ (aq) has Eºcell = 2.48 V.…

A: Given -> E°cell = 2.48 V pH = 2.00 [NI2+] = [ Ag+] = 0.030 M

Q: In a certain zinc-copper cell, Zn(s) + Cu2*(aq) → Zn2*(aq) + Cu(s) the ion concentrations are [Cu2+]…

A: Goven Zinc-Copper cell is Zn(s) + Cu2+(aq) ---> Zn2+(aq) + Cu(s) Concentration of Cu2+ , [Cu2+]…

Q: Use the Nernst equation to calculate the cell potential, EcellEcell, for a galvanic cell…

A: The half cell reactions are Pb+2 (aq)+ 2e− ⇌ Pb E° = –0.126 V Fe+2 (aq)+ 2e− ⇌ Fe (s) E° =…

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

A: Cell Notation : Zn(s) | Zn2+(aq,1M) || cu2+(aq, 1M) | Cu(s) Electrode potential of cathode = 0.34…

Question

In a certain zinc-copper cell,
Zn(s) + Cu2*(aq) → Zn2+(aq) + Cu(s)
the ion concentrations are [Cu2+] = 0.0234 M and [Zn2+] = 1.8 M.
What is the cell potential at 25 °C?
Ecell =
i
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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 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

Calculate the cell potential of a cell operating with the following reaction at 25°C, in which [Cr2O72− ] = 0.030 M, [I − ] = 0.020, M, [Cr3+ ] = 0.30 M, and [H+ ] = 0.50 M. Cr2O72-(aq) + 6 I −(aq) + 14 H+(aq) → 2 Cr3+(aq) + 3 I2(s) + 7 H2O(l)
Use the Nernst equation to calculate the cell potentials (in V) of the following cells at 298.15 K. 2+ (a) 2 Ag (aq, 0.20 M) + Ni(s) 2 Ag(s) + Ni (aq, 0.65 M) 2- (b) Pb(s) + SO₂ (ag, 0.30 M) + 2 AgCl(s) → PbSO4(s) + 2 Ag(s) + 2 C1 (ag, 0.20 M) (c) Sn(a) + SbCl, (ag, 0.10 M)→ Sn (aq, 0.20 M) + SbCl, (ag, 0.10 M) + 2 C1 (aq, 0.40 M)
What is the cell potential of the following electrochemical cell? (Report your answer to 2 significant figures.) Co(s) | Co²+ (aq, 0.31 M || Co²+ (aq, 0.035 M) | Co(s) Co²+/Co(s) = -0.28 V Eºred 1 2 4 7 +/- 5 8 v 3 6 9 0 X с x 100
Calculate the reaction temperature of the electrochemical cell described below which measures a potential of 0.313 V. Cu(s) | Cu2+ (0.80 M) || O2(g) (0.98 atm) | H+ (0.047 M), H2O2 (0.92 M) | Pt(s) (Use R = 8.314 J/mol-K; F = 96485 C/mol)
In a cell with an aluminum electrode in a solution of aluminum nitrate and a zinc electrode in a solution of zinc nitrate: Al|Al3+ || Zn2+|Zn. If you increase the concentration of Zn2+, which of the following is true about the cell potential?
In a certain zinc–copper cell, Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) the ion concentrations are [Cu2+] = 0.0218 M and [Zn2+] = 1.3 M.What is the cell potential at 25 °C?
The free energy change for the following reaction at 25 °C, when [Pb2+] = 3.82×10-3 M and [Cu2+] = 1.20 M, is 68.1 kJ: Pb2+(3.82×10-3 M) + 2Cu+(aq)Pb(s) + 2Cu2+(1.20 M) ΔG = 68.1 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?
Name: NetID: 5. Determine the standard cell potential (in V to two decimal places) for the following redox reactions. 2+ (a) Al(s) | Al³+ (aq, 1 M) || Cu²+ (aq, 1 M) | Cu(s) (b) Al(s) + NO3(aq) + 4H+ (aq) - Al³+ (aq) + NO(g) + 2H₂O(1) 13+ A: 2.00 A: 2.62
In a certain zinc-copper cell, Zn(s) + Cu2+(aq) → Zn2*(aq) + Cu(s) the ion concentrations are [Cu2+] = 0.0336 M and [Zn2+] = 1.8 M. What is the cell potential at 25 °C? Ecell = i V
An electrochemical cell consists of a silver metal electrode immersed in a solution with Ag* = 1.0 M separated by a porous disk from a copper metal electrode. If the copper electrode is placed in a solution of 5.0 MNH3 that is also 0.0080M in Cu(NH3),+, what is the cell potential at 25°C? Cu?+ (ag) + 4 NH3 (aq) = Cu(NH3)4²* (aq) K = 1.0 × 1013 Cell potential V
Consider the following galvanic cell: Agls) | Ag"(3.0 x 104 M)|| Fe*(1.1 x 10° M), Fe?-(0.040 M) | Pt(s) Choose the correct cell potential. O Ecel = + 0.12V O Ecel = - 0.15 V O Ecell = +0.09 V O Ecell = - 0.12 V Determine the sign of the electrodes in the cell. The left side half-cell is the and charged. The right side half cell is the and charged. Enter the equation for the spontaneous cell reaction. (Enter states of matter in your answer.) |
An electrochemical cell consists of a half-cell in which a piece of platinum wire is dipped into a solution that is 2.5 M in KI and 0.046 M in I2. The other half-cell consists of magnesium metal immersed in a 0.37 M Mg2+ solution. Assume that the temperature is 25°C. (a) Which electrode is the anode and which is the cathode? anode: Pt|I2, I- O Mg²+|Mg cathode: O Pt|I2, I- Mg2+|Mg (b) What is the emf of the cell? 4.0 2.869 X V (c) What is the spontaneous cell reaction? chemPad OHelp Greek - Mg2+(aq)+21 (aq) Mg(s)+I2(aq) Mg(s)+l_2(aq)-->Mg^2+(aq)+2l^-(aq) Your answer appears to have inconsistent states-of-matter. (d) What is the equilibrium constant of the cell reaction? 2.42e98