A galvanic cell is set up by making 1 M solutions of FeSO4 and ZnSO4, with an iron (Fe) electrode in the FeSO4 solution and a zinc (Zn) electrode in the ZnSO4 solution.   The half reactions that drive the galvanic cell are:    Fe2+ + 2e- → Fe      (at the cathode)               Zn  →  Zn2+ + 2e-    (at the anode) What happens to the mass of the Fe electrode while the cell runs?

The equilibrium constant of the reaction shown below is 2.41x10^8 at 25 degrees Celsius: 3Ag(s) + NO3-(aq) + 4H+(aq) --> 3Ag+(aq) + NO(g) + 2H2O(l) calxulte the value of Ecell for a cell utilizing this reaction

An electrochemical cell contains sodium chloride as a salt bridge and has the following line notation: X(s) | X* (aq) || Ag (aq) | Ag (s) (Note that X is a chemical that you will need to identify with oxidation state. +n) E° cell = 1.329 V a. Write the half-reaction that occurs at the anode and determine the E° anode. (Use the symbol X for now if this is the reaction at the anode). Write the half-reaction that occurs at the cathode and determine the E° cathode. (Use the symbol X for now if this is the reaction at the cathode). b. Identify the X(s)Xn* (ag) half-reaction and determine the Eo for this half-reaction.

A voltaic cell is constructed with two silver electrodes, each of which is based on the following half reaction: AgCl (s)  + e- -> Ag (s) + Cl- (aq) The two half cells have [Cl-] = 0.0150 M and [Cl-] = 2.55 M, respectively. Determine the overall reaction that takes place in the cell.

A voltaic cell employs the following redox reaction: 2 Fe3+ Calculate the cell potential at 25 °C under each of the following conditions. (ag) + 3 Mg (s) → 2 Fe (s) + 3 Mg²+ (aq) Part C [Fe+] = 3.10 M ; [Mg²+] = 1.2x10-3 M Ecell Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

a) Balance the following redox reaction in basic solution: H2O2(aq) + ClO2(aq) → ClO2-(aq) + O2(g) b) Sketch the voltaic cell for the redox reaction, labeling the direction for electron flow, the anode and cathode , and the species present in each half-cell. Show all the work please!

A voltaic cell is constructed in which the anode is a Al|Al3+ half cell and the cathode is a H2|H+ 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:     +              +     The cathode reaction is:     +              +     The net cell reaction is:     +              +     In the external circuit, electrons migrate     the H2|H+ electrode     the Al|Al3+ electrode.In the salt bridge, anions migrate     the Al|Al3+ compartment     the H2|H+ compartment.   Submit Answer Retry Entire Group 1 more group attempt remaining

Write the balanced equation of the reaction that occurs in a voltaic cell made using aluminum and tin electrodes immersed in 1.00 M solutions of Al3+ and Sn2+. Use the standard electrode potentials listed below to answer this question.

For the following galvanic cell, represented in line notation, determine what balanced half-reactions occur at each electrode. (Use the lowest possible whole number coefficients. Include states-of- matter under the given conditions in your answer.) Cd(s) | Cd2+(aq) I| Ni2+(aq) | Ni(s) anode half-reaction: chemPad Help XX"→ Greek cathode half-reaction: chemPad Help XX -> Greek DII F12 F11 F10 F9 80 888 F8 F7 F6 F6 F4 F3 esc F2 F1 & %24 5 6 7 8 3 4 1 T Y Q W G H J K 了 F. D. E 1L

Consider a voltaic cell in which the following reaction takes place. 2Fe 2+ (aq) + H₂O2 (aq) + 2 H+ (aq) --→2Fe ³+ (aq) +2H₂O (1) calculate Eº Calculate E and Gibbs free energy when [Fe²+] = 0.00813 M, [H₂O₂] = 0.914 M, [Fe ³+] = 0.199 M, [H] = 1.32 x 10³ M