(a) Calculate the emf of a cell made up of a hydrogen electrode ( P, = latm) and an oxygen electrode ( Po, = 0.5atm) in 0.5 M NaOH. (b) What is the polarity and which electrode is anode? (Assume that the oxygen electrode is reversible.)

(a) Calculate the emf of a cell made up of a hydrogen electrode ( P, = latm) and an oxygen electrode ( Po, = 0.5atm) in 0.5 M NaOH. (b) What is the polarity and which electrode is anode? (Assume that the oxygen electrode is reversible.)

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: A student measures Ecell of a concentration cell created by having the saturated solution of AgBr on…

A: According to the guidelines, we will solve the first 3 parts. If you want any other part also…

Q: Given the cell notation M1 | M12+(aq) | | M2+(aq) | M2, calculate the standard potential of the…

A: The cell given is, => M1 | M12+ (aq) || M2+ | M2 Given : Standard reduction potential of M1 =…

Q: To what pH should you adjust a standard hydrogen electrode toachieve an electrode potential of…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 210,…

Q: The permanganate ion, MnO4- , is a common oxidizing agent. What is the standard potential of the…

A: Standard reduction potential is the potential difference occurring between the cathode and anode. It…

Q: Consider the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M). The measured Ecell for…

A: Given that, the voltaic cell H+(aq, ?? M)|H2(g, 1 atm)||Cu(s)|Cu2+(aq. 0.1 M). So, [Cu2+] = 0.1 M,…

Q: (a) Write the anode and cathode reactions and the overall reaction occurring in a lead storage…

Q: (a) Calculate the emf of the following cell: Pt: Fe (activity = 0.1), Fe (activity = 0.001). Ag"…

Q: Calculate K for scandium fluoride, SCF3, given that the cell potential at 25 °C for the following…

Q: Calculate the maximum cell potential under these conditions. Show your work. Ecell = (round to 2…

A: we have to calculate Ecell

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

A: Given Ecell = 0.233V Ecell = - RTnFln [H+]0.233= - 8.314 x2981 x 96500ln [H+]- 9.075 = ln [H+] [H+]…

Q: A concentration cell is set up by connecting a half-cell containing a lead electrode in 0.10 M…

Q: How do I calculate the cell potential of this situation?

A: We have given a galvanic cell in which [Ti3+] = 0.02723 M [TiO2+] = 0.00146 M pH = 3 ESHE = 0.00V…

Q: Predict the standard potential for the galvanic cell. Standard reduction potentials can be found in…

A: Electrochemical cell is a cell in which chemical energy is converted into electrical energy. In this…

Q: Consider the following electrochemical cell:…

A: In electrochemical cell redox reaction occur

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

A: The given reaction is

Q: A student does an experiment to determine the molar solubility of lead(II) bromide. She constructs a…

Q: By what ratio will Q change if the cell potential is increased by 0.63 V? Assume v = 1 and the…

A: The electrode which has less negative reduction potential will act as a cathode and will undergo…

Q: Given a galvanic cell where one of the operating half reaction is: Pb (s) + 3 OH–(aq) ––––>…

Q: 7(a) The saturated calomel electrode (SCE) is a reference electrode based on the reaction between…

A: The balanced overall cell reaction can be obtained by combining the half-cell reactions. The…

Q: A student measures Ecell of a concentration cell created by having the saturated solution of AgBr on…

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.

Question

(a) Calculate the emf of a cell made up of a hydrogen electrode (P = latm)
and an oxygen electrode ( Po; = 0.5atm) in 0.5 M NaOH.
(b) What is the polarity and which electrode is anode? (Assume that the
oxygen electrode is reversible.)

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

For the reaction below, (a)construct a galvanic cell. Label the parts and the flow of electrons. Ca(s) + Cd2+(aq) --> Ca2+(aq) + Cd(s) (b) Write the cell notation/diagram for the above reaction. (c) Calculate the standard reduction potential of the cell and show the balanced chemical reaction. (d) Determine if the reaction will proceed spontaneously or not. Support your answer.
calculate the value of the electrode potential of hydrogen: a) in the 0.05 M solution of sulfuric acid, b) in the 0.05 M solution of potassium hydroxide
How would I calculate the cell potential?
The condensed cell diagram for the reaction occurring in silver–zinc button batteries is (-) Zn(s) | ZnO(s) | KOH(aq) || Ag2O(s) | Ag(s) (+) Write the halfreaction equation that involves silver.
The condensed cell diagram for the reaction occurring in silver–zinc button batteries is (-) Zn(s) | ZnO(s) | KOH(aq) || Ag2O(s) | Ag(s) (+) Write the halfreaction equation which involves zinc.
The electrodes in a silver oxide battery are silver oxide 1Ag2O2 and zinc. (a) Which electrode acts as the anode?
Based on the cell notation of an electrochemical cell, Pt(s) | H2 (g, 1 atm) | H+ (aq,0.02M)|| Ag* (aq.0.15 M) Ag (s) (a) write the half-cell notation equation of the anode and cathode. (b) write the overall cell reaction equation. (c) given that the cell potential is +0.852 V, calculate the standard reduction potential of silver. (d) calculate the equilibrium constant for the reaction at 25 C.
Consider the following electrochemical concentration cell at 25 oC: Ce3+(1 M)|Ce4+(0.01 M)||Ce4+(0.1 M)| Ce3+ (0.01 M) (a) calculate the electric force of the element (b) which electrode is the anode and which the cathode of the electrochemical cell? Given: the activity coefficients of Ce3+ and Ce4+ ions are equal to unity.
The following reaction occurs in an electrochemical cell: 3 HCIO,(aq) + 2 Cr³* (aq) + 12 H2O(e) → 3 HCIO(aq) + Cr,O? (aq) + 8 H;O* (aq) (a) Calculate AE° for this cell. (b) At pH 0, with [Cr,O;¯] = 0.80 M [HCIO,] = 0.15 M, and [HCIO] = 0.20 M, the cell potential is found to be 0.15 V. Calculate the concentration of Cr³*(aq) in the cell. %3D
(a) The standard reduction potential for X/X and Y/Y at 285 K are 0.52 V and 0.37 V respectively. (i) Express the half-reactions, overall reactions and the cell notation for this reaction. (ii) Distinguish if the reaction is spontaneous or non-spontaneous.
(2) What Zinc ion concentration is necessary for the actual cell potential to be (a) 0.250 volts, (b) 0.200 volts? Presume all other variables are at standard conditions. Zn +Cr Cr + Zn²+
To examine the effect of ion removal on cell voltage, a chemist constructs two voltaic cells, each with a standard hydrogen electrode in one compartment. One cell also contains a Pb/Pb21 half-cell; the other contains a Cu/Cu2+ half-cell.(a) What is Eo of each cell at 29o K?(b) Which electrode in each cell is negative?(c) When Na2S solution is added to the Pb21 electrolyte, solid PbS forms. What happens to the cell voltage?(d) When sufficient Na2S is added to the Cu2+ electrolyte, CuS forms and [Cu2+] drops to 1x10-16 M. Find the cell voltage.