A concentration cell was set up at 300 K using two hydrogen electrodes. If the cell is generating a potential of0.0387 V, answer the following questions:a) What is the concentration of H+ in the cathode's half-cell solution, if the anode's half-cell is 1 M?[H*]cat =number (rtol=0.03, atol=1e-08)b) What is the pH of the anode's half-cell solution, if the cathode's half-cell is 1.970 M?pH =number (rtol=0.03, atol=1e-08)c) What is Ecell when [H+]ano = 0.360 M and [H+]cat = 1.762 M?Ecellnumber (rtol=0.03, atol=1e-08)

a) To determine the concentration of H+ in the cathode half-cell reaction, For a concentration…

A concentration cell was set up at 300 K using two hydrogen electrodes. If the cell is generating a potential of 0.0387 V, answer the following questions: a) What is the concentration of H+ in the cathode's half-cell solution, if the anode's half-cell is 1 M? [H*Jcat = number (rtol=0.03, atol=1e-08) b) What is the pH of the anode's half-cell solution, if the cathode's half-cell is 1.970 M? pH = number (rtol=0.03, atol=1e-08) c) What is Ecell when [H+]ano = 0.360 M and [H†]cat = 1.762 M? Ecell number (rtol=0.03, atol=1e-08)

A concentration cell was set up at 300 K using two hydrogen electrodes. If the cell is generating a potential of 0.0387 V, answer the following questions: a) What is the concentration of H+ in the cathode's half-cell solution, if the anode's half-cell is 1 M? [H*Jcat = number (rtol=0.03, atol=1e-08) b) What is the pH of the anode's half-cell solution, if the cathode's half-cell is 1.970 M? pH = number (rtol=0.03, atol=1e-08) c) What is Ecell when [H+]ano = 0.360 M and [H†]cat = 1.762 M? Ecell number (rtol=0.03, atol=1e-08)

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 a cell described below, answer the questions that follow. (A). What would be the INITIAL cell…

A: In the given cell reaction, Zn(s) is undergoing oxidation, whereas Pb2+(aq) undergoes reduction to…

Q: Consider the following cell reaction at 23°C: Ca(s) + Cu+ Calculate the standard cell potential of…

A: Calculate the standard cell potential of the given cell,

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: A student measures the potential of a cell made up with 1 M CuSO4, in one solution and 1 M AgNO3, in…

Q: Suppose 30.0 mL of 0.100 M Pb(NO3)2 is added to 60.0 mL of 0.150 M KI. How many grams of Pbl2 will…

Q: Consider the following cell reaction: Cd(s) + 2 H*(? M) Cd2+ (1.00 M) + H2(g)(1.00 atm) If the cell…

A: To find the pH of the hydrogen electrode, we can use the Nernst equation:E cell = E∘ cell -…

Q: 10. Calculate the potential of the following cells: a) a galvanic cell consisting of a lead…

A: Given: Pb2+ =0.0848 MZn2+=0.1364 M TiO2+ =0.00146 M Ti3+ =0.02723

Q: 27

Q: A galvanic cell is established to power a torch, as shown.For this cell, the overall equation will…

A: The given cell diagram is : Options are : Overall cell equation for this reaction = ?

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

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: Consider the following cell notation and use a Table of Standard Electrode Potentials (Appendix Le…

A: Ecell can be calculated using nernest equation. To calculate Ecell , we would first write a complete…

Q: Consider the following cell reaction: Mn(s) + 2 H+(? M) Mn2+(1.00 M) + H2(g)(1.00 atm) If the cell…

A: Given data : Mn(s) + 2 H+(_____M) gives Mn2+(1.00 M) + H2(g)(1.00 atm)the cell potential (E cell…

Q: When the Ag* concentration is 1.36x10-4 M, the observed cell potential at 298K for an…

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

Q: Consider the following cell reaction: Cd(s) + 2 H*(? M) Ca2*(1.00 M) +H>(g)(1.00 atm) If the cell…

A: The cell reaction given is, Given: Cell potential = 0.186 V. And temperature = 298 K

Q: A galvanic cell is powered by the following redox reaction: 2+ 4 Cu (aq) + N,H(aq) + 4OH (aq) 4 Cu"…

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: 'red A certain half-reaction has a standard reduction potential E Eood = +0.40 V. An engineer…

A: Step 1:Galvanic cell is a type of electrochemical cell that converts chemical energy into electrical…

Q: What is the emf of this cell when [Fe2+] = 1.8 M, [Fe+] = 1.2x10-2 M , Po, = 0.55 atm , and the pH…

A: The voltaic cell reaction given is 4 Fe2+ (aq) + O2 (g) + 4 H+ (aq) → 4 Fe3+ (aq) + 2 H2O (l) The…

Q: Consider a galvanic cell for which the anode reaction is Pb(s) → Pb+2 (0.010 M) + 2e- , E= -0.1263…

A: According to guidelines we are supposed to answer only first three subparts. If you want rest of the…

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

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

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: 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

A concentration cell was set up at 300 K using two hydrogen electrodes. If the cell is generating a potential of
0.0387 V, answer the following questions:
a) What is the concentration of H+ in the cathode's half-cell solution, if the anode's half-cell is 1 M?
[H*]cat =
number (rtol=0.03, atol=1e-08)
b) What is the pH of the anode's half-cell solution, if the cathode's half-cell is 1.970 M?
pH =
number (rtol=0.03, atol=1e-08)
c) What is Ecell when [H+]ano = 0.360 M and [H+]cat = 1.762 M?
Ecell
number (rtol=0.03, atol=1e-08)

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

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

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

Consider the galvanic cell based on the following half-reactions. Ag+ + e− → Ag ℰ° = +0.80 V Fe2+ + 2 e− → Fe ℰ° = −0.44 V (a) Determine the overall cell reaction and calculate ℰ ° cell . (b) Calculate ΔG° and K for the cell reaction at 25°C. (c) Calculate ℰcell at 25°C when [Ag+ ] = 1.0 ✕ 10−4 M and [Fe2+ ] = 1.0 ✕ 10−2 M.
im a student plz help
Consider the galvanic cell based on the following half-reactions. Ag+ + e Ni²+ + 2e →→ Ni (a) Determine the overall cell reaction and calculate Omit states-of-matter from your answer.) chemPad XX→ (c) 8 cell → Ag 8⁰ = +0.80 V 8° -0.23 V Calculate 8 Help Greek º (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. AGO kJ K (in V). (Use the lowest possible whole number coefficients. cell (in V) at 25°C when [Ag+] = 1.0x10-4 M and [Ni²+] = 1.0×10-² M. cell V
Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to | the standard cell potentials on the last page of the note packet. Selected Answer: -54 A Calculate the AG° (in kJ) for the reaction of elemental chlorine with the bromide ion at 298K. Refer to the standard X cell potentials on the last page of the note packet. Selected Answer: 27.0
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.)
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
Cell Potential For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode: Ecell Ered (cathode) - Ed (anode) ▼ Tarnish on copper is the compound CuO. A tarnished copper plate i placed in an aluminum pan of boiling water. When enough salt is added so that the solution conducts electricity, the tarnish disappears. Imagine that the two halves of this redox reaction were separated and connected with a wire and a salt bridge. Part A Calculate the standard cell potential given the following standard reduction potentials: A²+ +3e Cu²+ + 20 Express your answer to two decimal places and include the appropriate units. ▸ View Available Hint(s) Ecell = li Value 4 → Units ? Al; E Cu; E 19 of 42 -1.66 V 0.340 V Review | Constants | Periodic Table
For the voltaic cell described by the cell reaction below, (1) write the cell diagram, (2) identify which specie is being reduced and which is being oxidized, (3) identify the anode and the cathode, (4) calculate the values of Q, and (5) using the table of standard reduction potentials, show the calculation of the Ecell using the Nernst equation [Ecell = E0cell – (0.0592/n x log Q)]. Zn + Ni+2 (0.10 M) → Zn+2 (0.30 M) + Ni
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.)