2. In another experiment, Fischl used chromium metal to form an electrode she can use for her voltaic cell. She wanted to determine theelectric potential produced by the chromium electrode (and 1.0 M of its corresponding electrolyte solution) with a Copper electrode in0.10 M CuSO4 solution at 25 °C. Predict the following:a. OHR of the voltaic cell:b. RHR of the voltaic cell:c. Number of electrons involved in the redox reaction (n):d. Overall reaction for the voltaic cell:e. Standard cell potential, E°cell:2Cr(s) + 3Cu^2+(aq) → 2Cr^3+(aq) + 3Cu(s)3Cr(s) + 2Cu^2+(aq) → 3Cr^3+(aq) + 2Cu(s)3Cr^3+(aq) + 2Cu(s) → 3Cr(s) + 2Cu^2+(aq)2Cr^3+(aq) + 3Cu(s) → 2Cr(s) + 3Cu^2+(aq)f. Theoretical Ecell :g. If the measured Ecell Was 0.75 V, calculate the percent error.%h. Oz suggested that they increase the concentration of CuSO4 solution used. What will be the effect on the measured potential?

“Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

2. In another experiment, Fischl used chromium metal to form an electrode she can use for her voltaic cell. She wanted to determine the electric potential produced by the chromium electrode (and 1.0 M of its corresponding electrolyte solution) with a Copper electrode in 0.10 M CuSO4 solution at 25 °C. Predict the following: a. OHR of the voltaic cell: b. RHR of the voltaic cell: c. Number of electrons involved in the redox reaction (n): eltais sellı

2. In another experiment, Fischl used chromium metal to form an electrode she can use for her voltaic cell. She wanted to determine the electric potential produced by the chromium electrode (and 1.0 M of its corresponding electrolyte solution) with a Copper electrode in 0.10 M CuSO4 solution at 25 °C. Predict the following: a. OHR of the voltaic cell: b. RHR of the voltaic cell: c. Number of electrons involved in the redox reaction (n): eltais sellı

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

2. In another experiment, Fischl used cadmium metal to form an electrode she can use for her voitaic cell. She wanted to determine the electric potential produced by the cadmium electrode (and 1.0 M of its corresponding electrolyte solution) with a Copper electrode in 0.10 CuSO4 solution at 25 °C. Predict the following: a. OHR of the voltaic cell: b. RHR of the voltaic cell: c. Number Cu^2+(ag) + 2e- → Cu(s), Eo = + 0.34 V d. Overall r Cd^2+(aq)+ 2e- → Cd(s), Eo = - 0.40 V e. Standar Cu(s) → Cu^2+(aq)+ 2e-, Eo = - 0.34 V f. Theoretic Cd(s) → Cd^2+(aq)+ 2e-, Eo = + 0.40 V % g. If the measured Ecell was 0.50 V, calculate the percent error. h. Oz suggested that they increase the concentration of CuSO, solution used. What will be the effect on the measured potential?
What is the minimum mass (in g ) of the cadmium that must be used to make the anode in this cell?
Answer no. 1
Hey im stuck on this sheet :) (no explanation or diagram needed)
C. d. b. e. f. 1. a. Consider the following reduction potential: Ag+ + le ----→ Ag E° = 0.34 V Zn+2 +2e ------- → Zn Eº= -0.76 V Balance the Redox reaction occurring in the cell What is the sum of the coefficients in the balanced equation and what is the number of electrons transferred? Identify the oxidizing agent in the reactions: Identify the specie/s found at the anode Determine the standard cell potential for the reaction Determine the value of the Gibbs free Energy for the reaction shal
Predict what is liberated at each electrode when aqueous solution of the following are electrolyzed between inert electrodes. Anode Product Cathode Product a. H:SO. b. K.SO, c. CusO. d. AuCl, e. KCi
A. From the reaction as shown below, calculate the Standard Cell Potential of a Galvanic Cell that uses the half-reactions shown below. Cr3+ + 3e- -------> Cr Eo = -0.73 V Al3+ + 3e- -------> Al Eo = -1.66 V B. A galvanic cell is made using 0.25M ZnSO4 and an unknown amount of CuSO4. The cell potential is 105V at 50oC. What is the concentration of CuSO4 in the cathode compartment? Zn(s) + Cu(aq)2+ -------> Zn(aq)2+ + Cu(s) Eo = 1.10 V Use:E = Eo - (RT/nF) + lnQ
inorganic chem question answer with explanation
3. How long will it take to electrodeposit 1.05 g Cr from 0.504 M Cr2O72- solution if 3.10 A current ispassed through the solution?A. 15082 s B. 1257 s C. 7541 s D. 2338 s E. 3770 s
#26
Consider the cell below. Please note that this cell may or may not obey the conventions of a standard cell diagram. Assume the cell is working spontancously under standard conditions. A B Salt bridge H. K. Image: Rectangle I in a beaker in a solution of J. An arrow F points away from rectangle I and an arrow E points toward rectangle I. The rectangle I is joined by a line another rectangle L in a separate beaker. On this line, an arrow labelled A points toward I and an arrow labelled B points to L. Rectangle L in a beaker in a solution of K. An arrow H points away from rectangle Land an arrow G points toward rectangle L.A salt bridge joins the beakers. On this salt bridge, an arrow labelled C points toward I and an arrow labelled D points to L. End of image. | = Q J = QNO3 Reduction Potential Q = minus 0.400 V K = RNO3 Reduction Potential R = minus 0.200 V L = R Match the each statement to the letter that best describes it. Some answers may be used more than once. of: C. E.
13.71 Round your answers to 6 decimal places