A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 0,(9)+4H (aq)+4e 2H,0() End = +1.23 V 3+ Fe (aq)+e - Fe (aq) E = +0.771 V red %3D 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.

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 0,(9)+4H (aq)+4e 2H,0() End = +1.23 V 3+ Fe (aq)+e - Fe (aq) E = +0.771 V red %3D 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.

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

BASIC PURE SUBSTANCE MIXTURE UNIT DESCRIPTION (color; physical state; transparent/translucent/opaque; shiny/dull malleable/ductile, shape and size of particles for solids; odor for organic series only) SAMPLE OF Соmpound (for Pure substances Element MATTER only) Homo- Hetero- atom, molecule, or formula unit Metal Nonmetal Ionic Covalent Series 8. ORGANIC CHEMICALS C,H14(1) Нехane HC,H3O2(aq) C4H3O2(1) ethyl acetate C;H60(1) Acetone CH,O(1) ethyl alcohol (ethanol) C10H3O(s) 1-naphthol C;H,O(1) Benzaldehyde C3H3O2(1) methyl benzoate C,H§O(I) trans-cinnamaldehyde
If a constant current of 2.0 amperes is passed through a cell containing Cr³+ for 1.0 hour, how many grams of Cr will plate out onto the cathode? (The atomic mass of Cr is 51.996.)
Please don't provide handwritten solution .....
+ 2+ MnO 4(aq) +8 H (aq) +5e → Mn(aq) + 4H₂O(1) 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. Answer the following questions about this cell. Do you have enough information to calculate the cell voltage under standard conditions? 3+ If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to significant digits. Fe half-reaction 0 (aq) + e Yes No V 2+ Fe (aq) standard reduction potential red 'red = +1.51 V = +0.771 V ローロ x 90 x10 S
Please explain and give the correct answers.
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2 H₂O(1)+2e →> H2(g)+2 OH (aq) E.ed = -0.83 V red Cu²+(aq)+e Cu+ (aq) →>> Answer the following questions about this cell. E° = +0.153 V red 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 ☐ ☐
A galvanic cell is powered by the following redox reaction: 2+ 2+ MnO₂ (s) + 4H* (aq) + Zn(s) Mn²+ (aq) + 2 H₂O(1) + Zn²+ (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 £ - Ov E V ローロ X G
Use the standard reduction potentials given below to predict if a reaction will occur between Ag(s) and F2 (g), when the two are brought in contact via standard half-cells in a voltaic cell. F2 (g)+2e7 →2F (aq) E red Agt (ag)+e → Ag(s) E red + = 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. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) - 2.870 V 0.799 V +
A constant current of 0.50 A is used to deposit copper at the cathode and oxygen at the anode of an electrolytic cell. What is the weight of copper (63.55 g/mol) formed after 10 minutes? F=96,485 C
Use the standard reduction potentials given below to predict if a reaction will occur between Zn(s) and Cl2(g), when the two are brought in contact via standard half-cells in a voltaic cell. | Cl2(g) + 2e¯¯ →2C1¯¯ (aq) E Zn2+ = 1.360 V red (aq) + 2e → Zn(s) E = = -0.763 V red 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. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + +
A galvanic cell is powered by the following redox reaction: 3 Br₂(1) + 2NO(g) + 4H₂O(1) - 6 Br (aq) + 2NO3(aq) + 8H (aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 0 E = v 00 Ś
An electrochemical cell is made of two electrodes: (Zn2+/Zn) and (Ag+/Ag). Use the standard reduction potentials to answer the following questions. What is the standard potential of the cell and which electrode is the cathode and which one is the anode? Write a net redox equation for this electrochemical cell.