Its counting it wrong, can u check and fix it. Im a students, idk if it may be the bottom part as well (to) (from). A voltaic cell is constructed in which the anode is a H₂| H* half cell and the cathode is a Br" | Br₂ half cell. The half-cell compartments are connected by a salt bridge.(Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.)The anode reaction is:H₂(g)2+The cathode reaction is:Br₂(g)+ 2eThe net cell reaction is:H₂(g)2+ Br₂(g)22H*(aq)2Br (aq)2H+ (aq)+An error has been detected in your answer. Check for typos,miscalculations etc. before submitting your answer.+2eEnter electrons as e.+ 2Br (aq)In the external circuit, electrons migrate from the H₂|H* electrode [toIn the salt bridge, anions migrate to the H₂|H* compartment from✓the Br | Br₂ electrode.the Br" | Br₂ compartment.

The electrode having less negative value of reduction potential acts as a cathode and the species…

A voltaic cell is constructed in which the anode is a H₂| H* half cell and the cathode is a Br | Br₂ half cell. The half-cell compartments are connected by a salt bridge. Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: H₂(g) The cathode reaction is: Br₂(g) + 2e The net cell reaction is: H₂(g) + Br₂(g) → - 2H*(aq) 2Br (aq) + 2e + 2H*(aq) + 2Br (aq) n the external circuit, electrons migrate from the H₂|H* electrode [to n the salt bridge, anions migrate to the H₂|H* compartment from ✓the Br Br₂ electrode. the Br Br₂ compartment.

A voltaic cell is constructed in which the anode is a H₂| H* half cell and the cathode is a Br | Br₂ half cell. The half-cell compartments are connected by a salt bridge. Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: H₂(g) The cathode reaction is: Br₂(g) + 2e The net cell reaction is: H₂(g) + Br₂(g) → - 2H(aq) 2Br (aq) + 2e + 2H(aq) + 2Br (aq) n the external circuit, electrons migrate from the H₂|H* electrode [to n the salt bridge, anions migrate to the H₂|H* compartment from ✓the Br Br₂ electrode. the Br Br₂ compartment.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section17.3: Voltaic Cells

Problem 17.3PSP

See similar textbooks

Similar questions

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?
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.
At 298 K, the solubility product constant for PbC2O4 is 8.5 1010, and the standard reduction potential of the Pb2+(aq) to Pb(s) is 0.126 V. (a) Find the standard potential of the half-reaction PbC2O4(s)+2ePb(s)+C2O42(aq) (Hint: The desired half-reaction is the sum of the equations for the solubility product and the reduction of Pb2+. Find G for these two reactions and add them to find G for their sum. Convert the G to the potential of the desired half-reaction.) (b) Calculate the potential of the Pb/PbC2O4 electrode in a 0.025 M solution of Na2C2O4.
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)
A standard galvanic cell is constructed so that the overall cell reaction is 2A13++(aq)+3M(s)3M2+(aq)+2A1(s) Where M is an unknown metal. If G = 411 kJ for the overall cell reaction, identify the metal used to construct the standard cell.
A voltaic cell is constructed using the reaction Mg(s) + 2H+(aq) Mg2+(aq) + H2(g) (a) Write equations for the oxidation and reduction half-reactions. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ______ half-cell to the ______ half-cell. The half-reaction at the anode is ____, and that at the cathode is _____.
The half cells Sn2+(aq) |Sn(s) and Cl2(g) |Cl(aq) are linked to create a voltaic cell. (a) Write equations for the oxidation and reduction half-reactions and for the overall (cell) reaction. (b) Which half-reaction occurs in the anode compartment, and which occurs in the cathode compartment? (c) Complete the following sentences: Electrons in the external circuit flow from the ______ electrode to the ____ electrode. Negative ions move in the salt bridge from the _____ half-cell to the _____ half-cell.
In principle, a battery could be made from aluminum metal and chlorine gas. (a) Write a balanced equation for the reaction thatwould occur in a battery using Al3+(aq) | Al(s) andCl2(g) | Cl(aq) half-cells. (b) Identify the half-reaction at the anode and at the cathode. Do electrons flow from the Al electrode when thecell does work? Explain. (c) Calculate the standard potential, Ecell, for the battery.
A half-cell that consists of a copper wire in a 1.00 M Cu(NO3)2 solution is connected by a salt bridge to a solution that is 1.00 M in both Pu3+ and Pu4+, and contains an inert metal electrode. The voltage of the cell is 0.642 V, with the copper as the negative electrode. (a) Write the half-reactions and the overall equation for the spontaneous chemical reaction. (b) Use the standard potential of the copper half-reaction, with the voltage of the cell, to calculate the standard reduction potential for the plutonium half-reaction.
The mass of three different metal electrodes, each from a different galvanic cell, were determined before and after the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes. The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, given the label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass. Make an educated guess as to which electrodes were active and which were inert electrodes, and which were anode(s) and which were the cathode(s).
Use the data from the table of standard reduction potentials in Appendix H to calculate the standard potential of the cell based on each of the following reactions. In each case, state whether the reaction proceeds spontaneously as written or spontaneously in the reverse direction under standard-state conditions. (a) H2(g)+Cl2(g)2H+(aq)+2Cl(aq) (b) Al3+(aq)+3Cr2+(aq)Al(s)+3Cr3+(aq) (c) Fe2+(aq)+Ag+(aq)Fe3+(aq)+Ag(s)
Give the notation for a voltaic cell whose overall cell reaction is Mg(s)+2Ag+(aq)Mg2+(aq)+2Ag(s) What are the half-cell reactions? Label them as anode or cathode reactions. What is the standard cell potential of this cell?