Answered: Calculate the cell emf for the…

Calculate the cell emf for the following reaction at 25°C: 2Ag (0.010 M) + H₂(1 atm) → 2Ag(s) + 2H*(pH = 10.0) Ag+ + e → Ag(s) Eº = +0.799 V 2H+ + 2e → H₂(g) Eº = 0,000 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: 2Cu²+ (aq) + Mg (s) →→→ 2Cu+ (aq) + Mg²+ (aq) Determine the equilibrium constant (K) of this…

A: The question is based on electrochemistry . we need to calculate equilibrium constant for the given…

Q: Consider the following reaction at 298 K. Pb?+ (aq) + Cu(s) → Pb(s) + Cu²+ (aq) Which of the…

Q: Consider the following unbalanced redox reaction that occurs in an electrochemical cell: Fe (s) +…

A: Given, Fe (s) + Al3+ (aq) -->Fe2+ (aq) + Al (s) standard gibbs free energy (∆G°) = ? Note:…

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

Q: Calculate E, and AG for the following cell reactions at 25 °C. [Mg 2+]= 0.032 M, [Sn 2+]=0.018 M…

A: Answer :- E = 2.22 V , ∆G = -429 kJmol…

Q: Compute the standard cell potential for the spontaneous reaction (ie. where Am(s) is being axidized)…

A: Reduction means the gain of electrons by species. Oxidation means the loss of electrons by a…

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

Q: n electrochemical cell is constructed in which both electrodes are pure iron immersed in a solution…

A: Solution - The correct option is (A)

Q: Calculate AGixn and Eo (cell

Q: State the cell that can be used to measure the equilibrium constant for the following reaction:…

A: Equilibrium is established when the rate of forward reaction becomes equal to the rate f backward…

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: According to Faraday's Law: W=ZIt ...... (1) where w is the mass formed, I…

Q: In the electrolysis of a 200 mL metal experiment, 0.0434 grams of cathode is applied when a current…

A: Given: weight of metal(w) = 0.0434 Current(I) = 0.50 A Time(t) = 5 min = 300 sec Valency factor =…

Q: Mg2"(aq) + 2 e Mg(s) E° = -2.38 V Cu2*(ag) + 2 e Cu(s) E° = +0.34 V O-2.04 V O +2.72 V O+2.04 V…

A: Given : Mg2+ (aq) + 2e- ==> Mg(s) E° = -2.38 V Cu2+ (aq) + 2e- ==> Cu (s) E° =…

Q: rent of 1.88 x 10° ampere is passed thro olytic cell for 24 hours. Calculate the m s9% efficient 80%

A: Charge = current × time Q = I × t Mass = M × Q / n × F M is the molar mass n is the number of…

Q: For the cell, H2(1 atm)|HBr(α=1)||AgBr|Ag, E is given as E = 0.07121 – 4.99 x 10-4 T – 3.45 x 10-6 T…

A: Given: E = 0.07121 – 4.99 x 10-4 T – 3.45 x 10-6 T2 T = 25 °C + 273 = 298 K

Q: Use the Nernst Eq. Ecell = Eocell - (RT/nF) lnQ to calculate the cell potential when [Mn2+] = 0.010…

A: Consider the following balanced redox reaction: Sn (s) + MnO2(s) + 4 H+(aq)→ Sn2+(aq)+ Mn2+(aq)+2…

Q: Consider the reaction of chlorine with manganese dioxide: 3 Cl2(s) + 2 MnO2(s) + 8 OH(aq) →6 Cr(aq)…

A: Given-> Equilibrium constant (Keq) = 6.63 × 1047

Q: An electrochemical cell is set up with the following configuration: Hg|Hg2+||Mn2+|Mn. The solutions…

A: Spontaneity of a Chemical reaction in a galvanic cell on the basis of cell potential:

Q: Calculate the free energy, ΔG°, (kJ/mol) for the galvanic cell performing the following reaction as…

A: The cell reaction given is V + Sr2+ → Sr + V2+ Temperature, T = 25 °C = (25 + 273.15) K = 298.15 K…

Q: A galvanic cell has the overall reaction: Zn(s) + 2Eu(NO3)3(aq) → Zn(NO3)2(aq) + 2Eu(NO3)2(aq) Which…

Q: An electrolysis cell contains X3+ ions. When a 5.45 A current is passed through the cell for 2.16 x…

A: In electrolysis cation is attracted towards cathode and anion is attracted towards to the anode.

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2MnO4 (aq)…

Q: Calculate the standard free energy, ∆G, for the electrochemical cell below. Is it a galvanic or…

A: Given that : Temperature = 298 K The oxidation half-reaction is : Pb(s) → Pb2+ Adding 2 electrons…

Q: galvanic cell formed from the following two half-reactions? Assume that the cell temperature is 38°C…

A: Galvanic cell reaction, Cd2+(aq) +Mg(s) --->Cd(s) + Mg2+(aq) E°cell = E°c - E°a = -0.403…

Q: When [Pb2+] = 1.47 M, the observed cell potential at 298 K for an electrochemical cell with the…

Q: When [Cu2+] = 1.37 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: Given-> [Cu2+] = 1.37 M T = 298 K Ecell =2.804 V

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: What is the equilibrium constant (K) and standard Gibbs energy (ΔG°) at 25°C for the following cell…

A: Note: None of the above given reaction is giving correct answer, but by assuming these two reaction…

Q: Use the attached picture to help answer the question. The image shows a galvanic cell with Ag as…

A: To answer the question : The image shows a galvanic cell with Ag as one electrode and Sn as the…

Q: Calculate the equilibrium constant, K at 25 °C for the reaction E cell = 1.53 V Zn2+ (aq) + 2 Fe2+…

A: We have to calculate the equilibrium constant for the given redox reaction.

Q: Calculate the free energy, AG°, (kJ/mol) for the galvanic cell performing the following reaction as…

A: Oxidation is the loss of electrons. Reduction is the gain of electrons. The reactions where…

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: 1)A voltaic cell is constructed, based on the Zn/Sn2+ ion reaction. Zn + Sn2+ → Zn2+ + Sn The…

A: We know that for any voltaic cell, the cell potential is given by : E = Eo - (RT/nF) ln Q Where Q=…

Q: When [Cu²+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: Given data: Cu2+ + Mg(s) -----> Cu(s) + Mg2+(aq) conc. of Cu2+ = 1.49M potential of cell = 2.806V…

Q: What is the standard cell potential (E° cell) for the spontaneous reaction between the half-cells…

A: Reduction takes place easily if the standard reduction potential is higher (positive) and oxidation…

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

A: Multiple questions

Q: When [Cu2+] = 1.49 M, the observed cell potential at 298 K for an electrochemical cell with the…

A: Given reaction is : Cu2+ (aq) + Mg (s) ------> Cu (s) + Mg2+ (aq) [Cu2+] = 1.49 M Non-standard…

Q: In the following: Al³+ (aq) + 3 e Al(s) E° = -1.66 V Cr³+ (aq) + 3e →→ Cr(s) E° = -0.74 V What is…

Q: Given: Br2 (1) + 2e 2 Br-1 12 (s) +2e=21-¹ O-1.63 V What is the standard cell potential for the…

A: The standard cell potential of any reaction is defined as the difference between the potential of…

Q: When the Hg2+ concentration is 8.04x10-4 M, the observed cell potential at 298K for an…

A: According to given questionfirst standard cell potential calculationsecond concentration calculation…

Q: If the concentration of Ag* is 0.0115 M, the concentration of H* is 0.355 M, and the pressure of H2…

A: Use Nernst equation, to get the cell potential:

Q: Given the following two half-reactions in basic solutions, determine which overall reaction is…

A: Cell potential can be determined from the equation; Ecell=Eocathode-EoanodeEocathode=reduction…

Q: E°cell

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

Q: Calculate the cell potential, at 298 K, for the following reaction under the conditions given.…

Question

Calculate the cell emf for the following reaction at 25°C:
2Ag (0.010 M) + H₂(1 atm) → 2Ag(s) + 2H*(pH = 10.0)
Ag+ e → Ag(s)
Eº = +0.799 V
2H+ + 2e → H₂(g)
Eº = 0,000 V

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 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 for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
For the galvanic (voltaic) cell 2+ - Fe(s) + Mn²+ (aq) → Fe²+ (aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²+] if [Mn²+] = 0.090 M and E = 0.78 V? Assume T is 298 K 1 4 7 +/- 2 LO 5 8 0.196 M 3 6 9 O X C x 100
Write the cell notation for an electrochemical cell consisting of an anode where Mg (s) is oxidized to Mg2+ (aq) and a cathode where Ag+ (aq) is reduced to Ag (s) . Assume all aqueous solutions have a concentration of 1 mol/L.
Consider the cell below at standard conditions: Zn(s) | Zn 2+ (aq) || Fe 2+ (aq) | Fe(s)Calculate the value of ΔG° for the reaction that occurs if the value of E° cell = 0.32 V for this cell.
Consider the following galvanic cell: Li (s) | 0.095M LiCl (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s) Using Appendix H in the textbook, determine the Ecell of this galvanic cell. 2.54 V - 2.88 V O -2.92 V 2.88 V 2.92 V
The chemical reaction that causes iron to corrode in air is given by: 4Fe+3O2→2Fe2O3 in which at 298 K, ΔHorxn = −1684 kJ and ΔSorxn = −543.7 J/K At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?
Can you break down the problem attached?
If the concentration of Ag+ is 0.0115 M, the concentration of H+ is 0.355 M, and the pressure of H2 is 1.00 atm, calculate the cell potential at 25.0°C.
Questions 20 and 21 refer to the following information. Galvanic Cell Cell Diagram E°cell (Volts) Mg | Mg2(1.0 M) || Pb*2(1.0 M) | Pb 1 2.24 Zn | Zn(1.0 M) || Pb*2(1.0 M) | Pb 2 0.63 Mg | Mg*(1.0 M) || Zn*2(1.0 M) | Zn 3 The chemical reaction occurring in first galvanic cell is: Mg + Pb*2 → Mg+2 + Pb 21. If the concentration of Mg+2 is changed from 1.0 M to 3.0 M in the galvanic cells above, what will happen to the observed cell voltages in galvanic cells 1 and 3? (A) The voltage in both galvanic cells 1 and 3 will increase. (B) The voltage will decrease in both galvanic cells 1 and 3. (C) The voltage in galvanic cell 1 will increase and will decrease in galvanic cell 3 (D) The voltage in galvanic cell 3 will increase and will decrease in galvanic cell 1. 22. Consider a voltaic cell based on these half-cells. Ag (aq) +e → Ag/s) Cd (aq) + 2e → Cd¢s) E* = +0.80 V E = -0.40 V Identify the anode and give the voltage of this cell under standard conditions. (A) Ag; Ecell = 0.40 V (B) Ag;…
The free energy change for the following reaction at 25 °C, when [Hg²+] = 1.20 M and [Pb2+] = 7.55x10-3 M, is -202 kJ: Hg2+(1.20 M) + Pb(s) Hg(l) + Pb2+(7.55×10-3 M) AG = -202 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? forward or reverse
Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode. MnO4- + H+ + Ce3+ -> Ce4+ + Mn2+ + H2O
Consider the following half reactions: M²+ (aq) + 2e (aq) → M(S) X³+ (aq) + 3e (aq) →→→→→→X(s) Eº=-0.4 Eº=-0.7 Calculate the overall cell potential for the overall spontaneous redox reaction. Give your answer to one decimal place.