Question

A student measures the potential of a cell made up with 1.0 M CuSO4 in one...

A student measures the potential of a cell made up with 1.0 M CuSO4 in one solution and 1.0 M AgNO3 in the
other. There is a Cu electrode in the CuSO4 and a Ag electrode in the AgNO3. A salt bridge connects the 2
half cells. The student finds that the potential, or voltage of the cell, E°cell is 0.45 V and that the Cu electrode is
negative.
a. At which electrode is the oxidation occurring? ___________
b. Write the equation for the oxidation reaction.
c. Write the equation for the reduction reaction.
d. Write the overall equation for the reaction.
e. The student adds 6.0 M NH3 to the CuSO4 solution until the Cu2+ ion is essentially all converted to
Cu(NH3)42+ ion. The voltage of the cell, Ecell, goes up to 0.92 V and the Cu electrode is still negative.
Find the residual concentration of Cu2+ ion in the cell. (Use the Nernst Equation)
__________

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s)...
Use the standard reduction potentials shown here to answer the questions. Reduction half-reaction E∘ (V) Cu2+(aq)+2e−→Cu(s) 0.337 2H+(aq)+2e−→H2(g) 0.000 A copper, Cu(s), electrode is immersed in a solution that is 1.00 M in ammonia, NH3, and 1.00 M in tetraamminecopper(II), [Cu(NH3)4]2+. If a standard hydrogen electrode is used as the cathode, the cell potential, Ecell, is found to be 0.073 V at 298 K. Part A Based on the cell potential, what is the concentration of Cu2+ in this solution?...
A student dips a copper electrode (cathode) into a beaker containing 1M CuSO4 solution and a...
A student dips a copper electrode (cathode) into a beaker containing 1M CuSO4 solution and a silver electrode (anode) in another beaker containing 1M AgNO3 solution, a salt bridge containing Na2SO4 connecting the two beakers. The measured voltaic cell potential is + 0.42Volt a. What happens at the cathode and at the anode b. Write the equation of the cell reaction that occurs c. Write down the cell notation d. In the voltaic cell experiment above, explain the fundamental differences...
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+ +...
A concentration cell is made up of the Cu2+/Cu couple, where the Cu2+ concentrations are 1.0M...
A concentration cell is made up of the Cu2+/Cu couple, where the Cu2+ concentrations are 1.0M and 0.10 M. It follows that the anode compartment contains the ________ which _______ in concentration as the cell operates, and the cathode compartment contains the ________ which _______ in concentration as the cell operates. (a) 0.10 M Cu2+ solution, decreases; 1.0 M Cu2+ solution, also decreases (b) 0.10 M Cu2+ solution, increases; 1.0 M Cu2+ solution, decreases (c) 0.10 M Cu2+ solution, decreases;...
Predict the potential for the following voltaic cell at 25 C: Cu(s)|CuSO4(0.42 M)||AgNO3(0.46 M)|Ag(s) (answer in...
Predict the potential for the following voltaic cell at 25 C: Cu(s)|CuSO4(0.42 M)||AgNO3(0.46 M)|Ag(s) (answer in volts)
A) A student mixes in a test tube 3.00mL of 0.050M CuSO4 with 7.00mL of 0.20M...
A) A student mixes in a test tube 3.00mL of 0.050M CuSO4 with 7.00mL of 0.20M NH3/NH41+. The solution becomes a deep blue color. Assuming all the Cu2+ is complexed with NH3 to form the [Cu(NH3)4]2+ ion, determine the concentration of the complex in the solution. B) The standard solution made in question #1 was then scanned and the wavelength of maximum absorbance was determined. At the wavelength of maximum absorbance (minimum %T) the %T was found to be 12.16%....
A galvanic (voltaic) cell consists of an electrode composed of magnesium in a 1.0 M magnesium...
A galvanic (voltaic) cell consists of an electrode composed of magnesium in a 1.0 M magnesium ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found here.
The concentrations of NaCl and KI are at 0.150 M and 0.100 M, respectively, in the...
The concentrations of NaCl and KI are at 0.150 M and 0.100 M, respectively, in the following electrochemical cell: A) Using the following half-reactions, calculate cell voltage: CuI(s) e- ----> Cu(s)I- Eo=-.185 AgCl(s) +e- ----> AgCl- Eo=.222 E=? hint:Part A is solved by calculating the half-cell potential for the right and left half-cell. Use the Nernst equation and the concentration of the counter ion (Cl– or I–) to find each half-cell potential. There is only one electron involved in these...
Metal/Metal Ion Predicted Potential (V) Ag(s) | Ag+(1.0 M, (aq)) Ag(s) | AgCl(s) | Cl- (1.0...
Metal/Metal Ion Predicted Potential (V) Ag(s) | Ag+(1.0 M, (aq)) Ag(s) | AgCl(s) | Cl- (1.0 M, (aq)) Zn(s) | Zn2+ (1.0 M, (aq)) Pb(s) | Pb2+ (1.0 M, (aq)) Cu(s) | Cu2+ (1.0 M, (aq)) The predicted potentials are the ones you expect to measure using Ag(s) | AgCl(s) | Cl- (3.0 M(aq)) reference electrode. Please help! and make sure to explain so i can learn what is going on! Thanks.
A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M iron(II)...
A galvanic (voltaic) cell consists of an electrode composed of iron in a 1.0 M iron(II) ion solution and another electrode composed of silver in a 1.0 M silver ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Standard reduction potentials can be found here (https://sites.google.com/site/chempendix/potentials)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT