ghing a galvanic cell from two half-reactionsWrite a vuiuncedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode.Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction isspontaneous aswritten.Do you haveenoughinformation tocalculate the cellYesvoltage understandardconditions?NoIf you said it waspossible tocalculate the cellvoltage, do so andenter your answer Vhere. Round youranswer to 2CheckExplanation22 A chemist designs a galvanic cell that uses these two half-reactions:half-reactionstandard reduction potentialBr,(1)+2e2 Br (aq)E=+1.065 V||'red2+MnO2(s)+4H (aq)+2e- Mn"(aq)+2 H,O(1)= +1.23 VredAnswer the following questions about this cell.Write a balancedequation for thehalf-reaction thathappens at thecathode.Write a balancedequation for thehalf-reaction thathappens at theanode,Write a balancedequation for theoverall reactionthat powers thecell. Be sure thereaction is

Answered: Image /qna-images/answer/7e27fb87-d656-48f5-ac13-6bbb61c403fb.jpg

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e 2 Br (aq) =+1.065 V red 2+ MnO,(s)+4 H (aq)+2e Mn"(aq)+2 H,O(1) = +1.23 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

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e 2 Br (aq) =+1.065 V red 2+ MnO,(s)+4 H (aq)+2e Mn"(aq)+2 H,O(1) = +1.23 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

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 14P

See similar textbooks

Similar questions

The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
For each of the reactions, calculate E from the table of standard potentials, and state whether the reaction is spontaneous as written or spontaneous in the reverse direction under standard conditions. (a) Zn(s)+Fe2+(aq)Zn2+(aq)+Fe(s) (b) AgCl(s)+Fe2+(aq)Ag(s)+Fe3+(aq)+Cl(aq) (c) Br2(l)+2Cl(aq)Cl2(g)+2Br(aq)
a Calculate G for the following cell reaction: Tl(s)Tl+(aq)Pb2+(aq)Pb(s) The Gf for Tl+(aq) is 32.4 kJ/mol. b From G, calculate the standard cell potential for the cell reaction and from this, determine the standard potential for Tl2+(aq)+eTl(s).
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
At 298 K, the solubility product constant for solid Ba(IO3)2 is 1.5 109. Use the standard reduction potential of Ba2+(aq) to find the standard potential for the half-reaction Ba(IO3)2(s)+2eBa(s)+2IO3(aq)
Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?