Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Transcribed Image Text: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.
no minimum
yes, there is a maximum.
no maximum
0
E 0V
red
0
E
red
=
=
☐v
Transcribed Image Text:A certain half-reaction has a standard reduction potential E -0.89 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that
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 cathode of the cell.
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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 Varrow_forwardA 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.arrow_forwardWrite 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. 中 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 voltage under standard conditions? O О If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits. Ον No Yes ローロ e ☐ x10 Garrow_forward
- 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…arrow_forwardZinc 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.arrow_forwardHelp with the following question The 2nd photo is a close uparrow_forward
- The answer is supposed to be in gramsarrow_forwardby: 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?arrow_forwardUse 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.arrow_forward
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