Question

While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used...

While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used electrodes to monitor the cell potential. Using the table of theoretical values and what you know of the metals to fill in the blanks below.

When writing equations: Use spaces only before and after a plus sign. For example, the reaction: Fe2++2e−→FeFe2++2e-→Fe  would be entered as: Fe^2+ + 2e^- →→ Fe

Galvanic Cell Consisting of: Cu2++2e− →→ Cu 0.34
Zn2++2e− →→ Zn -0.76
E0cell Measured 0.95
Write the equation occuring at the anode. →→  
Write the equation occurring at the cathode. →→   
Shorthand Notation for the Cell: l  lI  l
Oxidizing Agent:

Zn

`Zn2+

Cu

Cu2+

Reducing Agent:

Zn

Cu

`Zn2+

Cu2+

E0cell from Table Values (Theoretical Numbers above).
E0cell Percent Error

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used...
While performing Lab 11, Electrochemistry, students connected 1 M solutions of the following metals and used electrodes to monitor the cell potential. Using the table of theoretical values and what you know of the metals to fill in the blanks below. When writing equations: Use spaces only before and after a plus sign. For example, the reaction: Fe2++2e−→FeFe2++2e-→Fe  would be entered as: Fe^2+ + 2e^- →→ Fe Galvanic Cell Consisting of: Zn2++2e− →→ Zn -0.76 Mg2++2e− →→ Mg -2.37 E0cell Measured...
Electrochemical Cell Potentials Table 1: Electrochemical Cell Potentials Cell Measured Total Potential from Multimeter (V)1 Individual...
Electrochemical Cell Potentials Table 1: Electrochemical Cell Potentials Cell Measured Total Potential from Multimeter (V)1 Individual Half-Cell Potentials Cell Reactions5 ΔG (kJ)6 (Cu) Electrode Standard Potential (V)2 Metal Electrode Experimental Potential (V)3 Metal Electrode Theoretical Potential (V)4 Metal Electrode Potential % Error Cu | Sn 0.469 0.34 V 0.34-0.469 =-0.129 Cathode:       Cu2+ + 2e- -> Cu Anode:            Sn ->Sn2++ 2e- Net:          Cu2+ + Sn -> Cu + Sn2+ Cu | Al 0.796 0.34 V 0.34-0.796 =-0.456 Cathode:   Cu2+ +...
CAn someone please let me know if my answers are correct Exercise 1: Construction of a...
CAn someone please let me know if my answers are correct Exercise 1: Construction of a Galvanic Cell Data Table 1. Spontaneous Reaction Observations. Metal in Solution Observations Zinc in Copper Sulfate Zinc turned black Copper in Zinc Sulfate There was no change Data Table 2. Multimeter Readings. Time (minutes) Multimeter Reading (Volts) 0 1.08 15 1.08 30 1.08 45 1.08 60 1.08 75 1.08 90 1.08 105 1.08 120 1.05 135 1.04 Data Table 3. Standard Cell Potential. Equation...
1. You titrate a 10.00 mL sample of a solution of borax with HCl. If it...
1. You titrate a 10.00 mL sample of a solution of borax with HCl. If it requires 24.89 mL of 0.100 M HCl to reach the endpoint, calculate Ksp for borax. ______M 2. Considering the information given and the calculations performed, how many significant figures should properly be reported for the answer to the previous question. A. 2 B. 3 C. 4 D. 5 3. You measure Ksp for borax to be 7.8 x 10-3 and 2.9 x 10-3 at...