Data Table 4Standard Reduction PotentialsReduction Half Reaction e° (v)Cu2+ + 2e → Cu0.34Pb2+ + 2e → Pb-0.13Zn2+ + 2e → Zn-0.76Mg2+ + 2e → Mg-2.37Student Questions1. For each of the three cells, write a shorthand cell notation.2. Using data table 4, assign the identities of each of the metals (A-D).3. Using the identity of Metal A, adjust the half-cell potentials to make them standardreduction potentials.4. From least to most active, list the metals in this experiment.Page 6 of 61155 wordsEI Focus143%

“Since you have asked multiple questions, we will solve the first question for you. If you want any specific question to be solved then please specify the question number or post only that question.” Cell notation is a way of representing the actual reactions that take place in an electrochemical cell by mentioning the participating components in each half cell. In a complete cell, the anodic and cathodic compartment is separated by a salt bridge and the anodic half cell situates on the left and the cathodic half cell positions on the right side. Appropriate notations such as s, l, and g to represent the solid, liquid, and gas phase of the half cell components are employed. The concentration of the solution is shown inside the parentheses. Since the reduction potential of the half cell components is provided, all the half cell reaction is considered to undergo reduction. Let the concentration of the solution be x M. Cell notations: i) Cu2+aq(x M)|Cus e°=0.34 Vii) Pb2+aq(x M)|Pbs e°=-0.13 V iii) Zn2+aq (x M)|Zns e°=-0.76 Viv) Mg2+aq (x M)|Mgs e°=-2.37 V The aqueous phase is represented by 'aq' and the separation of the electrode and the electrolyte solution is denoted by '|' line. The concentration of the solution is expressed inside the parentheses as x M.Hence the cell representation of each half cell is furnished.

Science

Chemistry

Data Table 4 Standard Reduction Potentials Reduction Half Reaction e° (v) Cu2+ + 2e → Cu 0.34 Pb2+ + 2e → Pb -0.13 Zn2+ + 2e → Zn -0.76 Mg2+ + 2e → Mg -2.37 Student Questions 1. For each of the three cells, write a shorthand cell notation.

Data Table 4 Standard Reduction Potentials Reduction Half Reaction e° (v) Cu2+ + 2e → Cu 0.34 Pb2+ + 2e → Pb -0.13 Zn2+ + 2e → Zn -0.76 Mg2+ + 2e → Mg -2.37 Student Questions 1. For each of the three cells, write a shorthand cell notation.

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

Similar questions

Question 25 Consider the electrochemical cell diagram shown below. As you observe the reaction in the cell, you notice that the manganese electrode seems to be disappearing while there are deposits forming on the cadmium electrode. Which of the following is a correct statement? Cd CaSO4(aq) 1M CdS04 Mn 1M MnSO4 beakerCdMn.gif The half-reaction occurring at the manganese electrode is Mn²+ + 2e →Mn. Electrons are flowing from the cadmium electrode to the manganese electrode. Sulfate ions are flowing through the salt bridge to the manganese solution. If this cell were used as a battery, the cadmium electrode would be marked "-".
Balance the following, Oxidation reduction reaction in aqueous acid. Please do parts D-F. H2O2(aq) + Hg(S)→ Hg2+2(aq) + H2O(l) a)Draw a picture of this cell label the anode and cathode. Show all necessary parts (label). Show the direction electrons, + ions and – ions flow/ b)Write the shorthand notation for this cell. c)Using the attached table calculate E0cell for this reaction d)What is the number of moles of electrons transferred in this reaction? e)Calculate the standard state change in Gibb’s free energy for this cell. f)If the concentrations are [H2O2(aq)] = 1.00 M, [Hg2 +2]= 0.100 M and pH = 2.75 what is Ecell for this reaction at 25 celsius?
In the electrochemical cell using the redox reaction below, the anode half reaction is ________.Sn4+(aq) + Fe (s) →→ Sn2+ (aq) + Fe2+(aq) Fe+2e−→Sn2+ Fe+2e−→Fe2+ Sn4++2e−→Sn2+ Fe→Fe2++2e− Sn4+→Sn2++2e−
Balance each of the following half- cell reactions in basic solution. NO3^ - -----> NH^4+
Determine the reduction/oxidation reactions and the rest of the textbook question
The diagram below shows a voltaic cell. The anode is Electrode A Component C V Component D Direction E Electrode B Direction F Direction of electron flow Select one: ○ Electrode A ○ Electrode B O Component C ?
Enter your answer in the provided box. Calculate the emf of the following concentration cell: Mg(s) | Mg*(0.37 M) || Mg*(0.77 M) | Mg(s) V
Consider a galvanic cell created from the following redox reaction: 3Zn (s) + 2Au3+ (aq) → 3Zn2+ (aq) + 2Au (s) 1) Draw out a schematic diagram (as shown in image) 2) Label each component (anode, cathode, salt bridge, solution choice, and electron flow direction) in your schematic diagram.
Answers for Question 2 and 3 please.