Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell. Note: write the half reaction as it would actually occur at the anode. Oyes, there is a minimum. O no minimum 0 yes, there is a maximum. no maximum 0 E red = Ov 0 E = v red

Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell. Note: write the half reaction as it would actually occur at the anode. Oyes, there is a minimum. O no minimum 0 yes, there is a maximum. no maximum 0 E red = Ov 0 E = v red

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...

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A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2 IO3(aq)+12 H*(aq)+10e¯ 1₂(s) + 6H₂O(1) 2+ Cu²+ (aq)+e Cu (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to calculate the cell Yes 1 standard reduction potential = +1.195 V Ered red = +0.153 V
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2 H,O(1)+2e H,(9)+2ОН (аq) E red -0.83 V Cu"(aq)+e 2+ - Cu (aq) End=+0.153 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
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0 A certain half-reaction has a standard reduction potential E 'red must provide at least 0.70 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the cathode of this cell. Note: write the half reaction as it would actually occur at…
Zinc is used as a “sacrificial” anode on hulls of salt water vessels made of iron. The effectis to reverse the oxidation of iron to iron (II) by causing zinc to oxidize to the zinc ion. Calculate the voltage for this reaction if it takes place under standard conditions.
Help with the following question The 2nd photo is a close up
The answer is supposed to be in grams
by: Th The concentration cell to the left was allowed to operate until the cell reaction reached equilibrium. What are the cell potential and the concentrations of zinc(II) in each half-cell for the cell now?
Use smallest possible integer coefficients. If a box is not needed, leave it blank. Use a table of Standard Reduction Potentials to predict if a reaction will occur between Hg metal and I,(s), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.
please include units in the answer