Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e + Mn e° = -1.18 V Fe?+ + 2e¯ - Fe ɛ° = -0.44 V a. Determine the overall cell reaction and calculate e: (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + Ecell b. Calculate AG° and K for the cell reaction at 25°C. AG° kJ K = c. Calculate Ecell at 25°C when Mn²+ = 0.10 M and = 6.7 x 10-5 M. Ecell =

Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e + Mn e° = -1.18 V Fe?+ + 2e¯ - Fe ɛ° = -0.44 V a. Determine the overall cell reaction and calculate e: (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + Ecell b. Calculate AG° and K for the cell reaction at 25°C. AG° kJ K = c. Calculate Ecell at 25°C when Mn²+ = 0.10 M and = 6.7 x 10-5 M. Ecell =

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

Consider the galvanic cell based on the following half-reactions: Mn2+ + 2e → Mn ɛ° -1.18 V Cd2+ + 2e –→ Cd e° : -0.40 V = a. Determine the overall cell reaction and calculate cell · (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + + E cel b. Calculate AG° and K for the cell reaction at 25°C. AG° kJ K C. Calculate Ecell at 25°C when Ma*] Ca*+ = 1.2 Mn²+ - 0.10 М and x 10-5 М. Ecell =
A voltaic cell is constructed in which the anode is a Fe|Fe2+ 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 (from or to?) the H2|H+ electrode (from or to?) the Fe|Fe2+ electrode.In the salt bridge, anions migrate (from or to?) the Fe|Fe2+ compartment (from or to?) the H2|H+ compartment.
Consider the galvanic cell based on the following half-reactions. Ag+ + e → Ag Cd²+ + 2e →→ Cd (a) Determine the overall cell reaction and calculate º chemPad XX² cell 8° = +0.80 V 8⁰ = -0.40 V V AGO K Help Greek (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. kJ (in V). (Use the lowest possible whole number coefficients. Omit states-of-matter from your answer.) cell (c) Calculate cell (in V) at 25°C when [Ag+ ] = V 1.0×10-4 M and [Cd²+] = 1.0×10-² M.
A voltaic cell is constructed in which the anode is a Cr | Cr³+ half cell and the cathode is a Cu| Cu²+ 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: J - Enter electrons as e. - In the external circuit, electrons migrate In the salt bridge, anions migrate ( the Cu Cu2+ electrode | the Cr| Cr³+ compartment [ the Cr| Cr³+ electrode. the Cul Cu2+ compartment.
Consider the galvanic cell based on the following half-reactions: Zn+ + 2e + Zn e° = -0.76 V Cd²+ + 2e → Cd e° = -0.40 V a. Determine the overall cell reaction and calculate e (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (5). If a box is not needed, leave it blank.) b. Calculate AG° and K for the cell reaction at 25°C. AG kJ K = [Zn**] = 0.10 M and [Ca] = c. Calculate e cell at 25°C when Zn 1.2 x 10-5 M. Ecell =
Use the Nernst equation to determine the cell potential, Ecell, of the galvanic cell consisting of the following half-cell systems: Ag+(0.010M) + e- --> Ag Eo= +0.80 V Cr3+(O.010M) + 3e- --> Cr Eo= -0.74 V
ISTRY (References] Consider the galvanic cell based on the following half-reactions: Zn+ + 2e- Zn e =-0.76 V Fe+ + 2e→ Fe e = -0.44 V a. Determine the overall cell reaction and calculate eI (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (5). If a box is not needed, leave it blank.) E = b. Cafculate AG° and K for the cell reaction at 25°C. AG C. Calculate Ecell at 25°C when Zn = 0.10 M and Fe 8.0 x 10 6 M. Erell =
2+ 2+ A voltaic cell is constructed from a standard Sn²+ Sn half cell (E° red = -0.140V) and a standard Fe³+ Fe²+ half cell (E° red = 0.771V). (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 spontaneous cell reaction is: + The cell voltage is V. ↑ 1 ↑ + + +
A voltaic cell is constructed that uses the following half-cellreactions:Cu+(aq) + e- ----->Cu(s)I2(s) + 2 e- ----->2 I-(aq)The cell is operated at 298 K with [Cu+] = 0.25 M and[I-] = 0.035 M. (a) Determine E for the cell at these concentrations.(b) Which electrode is the anode of the cell?(c) Is the answer to part (b) the same as it would be if the cellwere operated under standard conditions? (d) If [Cu+] wereequal to 0.15 M, at what concentration of I- would the cellhave zero potential?
Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these
3. The Eel fora galvanic cell composed of a Li electrode and an unknown electrode was found to be 2.91 volts. Use the Standard Reduction Potential table to determine the identity of the unknown electrode. Show work. Ered (Volts) -0.80 -0.34 -0.04 -0.76 -0.14 -0.40 -2.37 Half-Reaction Ag (aq) + 1e → Ag(s) Cu²+ (aq) + 2e > Cu(s) Fe (aq) + 3e > Fe(s) Zn²+ (aq) Sn²+ (aq) + 2e +2e → Zn(s) Sn(s) Cd²+ (aq) + 2e* Cd(s) Mg²+ (aq) + 2e Mg(s)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 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.