Co (s) | Co2+ (aq) || Au3+ (aq) | Au (s)
Q3\ For the previous cell, determine the concentration of the cobalt ion when a cell voltage of 1.76 V is obtained using a 0.761 M gold (III) nitrate solution.
Q4\ Calculate the free energy for the nonstandard cell in the previous problem. Show all work. Be mindful of signs, sig figs, and units
Q5\ Consider a galvanic cell consisting of the following two redox couples: Sn2+ (aq, 0.010 M) + 2e- --> Sn (s) Eo = -0.14 V Cs+ (aq, 0.010 M) + e- --> Cs (s) Eo = -2.92 V
a. Write the equation for the half-reaction at the cathode
b. Write the equation for the half-reaction at the anode
c. Write a shorthand cell notation version of this battery
d. Calculate the standard cell potential for this battery in volts. Include the correct number of sig figs in your answer.
Co (s) | Co2+ (aq) || Au3+ (aq) | Au (s) Q3\ For the previous cell,...
Calculate the cell potential for the galvanic cell in which the reaction Fe(s)+Au3+(aq)−⇀↽− Fe3+(aq)+Au(s) occurs at 25 ∘C , given that [Fe3+]=0.00150 M and [Au3+]=0.795 M . Refer to the table of standard reduction potentials. E= V
pleas help me with lab assament
Multimeter Consider a galvanic cell consisting of the following two redox couples: Ag+(0.010 M) + e-→ Ag(s) Eo = +0.80 V oi a. Write the equation for the half-reaction occurring at the Salt bridge C (0.010 M) Ag (0.010AM b. Write the equation for the half-reaction occurring at the anode. Cr Ag c. Write the equation for the cell reaction. d. What is the standard cell potential, Eelli for the cell? e. Realizing the...
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The E°nickel = -0.25 V and E°mercury = 0.789 V. (blank 1) Write the balanced reaction that occurs at the anode. (blank 2) Write the balanced reaction that occurs at the cathode. (blank 3) Calculate the standard cell potential of this galvanic cell. (blank 4) Write the shorthand cell notation for the galvanic cell. Question 10 options: Blank # 1 Blank # 2 Blank #...
please solve A to d to get thumps up.
Question 11 5 pts Consider a galvanic cell consisting of the following two redox couples: Sn2+ (aq, 0.010 M) + 2e --> Sn (s) E.-0.14 V Cst (aq, 0.010 M) + e --> Cs(s) E--2.92 V a. Write the equation for the half-reaction at the cathode Question 12 5 pts b. Write the equation for the half-reaction at the anode HTML Editor Question 13 6 pts c. Write a shorthand cell...
A galvanic cell based on the following reactions Cu 2+ (aq) + 2e- + Cu(s) E°=0.339 V (AD + 14H(aq) + 6e-4 2Cr 3+(aq) + 7 H2O(1) Eo=1.330 V a) Write the overall cell reaction and determine its voltage. b) If the E value of the galvanic cell is 1.2 le of the galvanic cell is 1.254 V, calculate the pH of the cell when [Cu2+]=0.00010 M, Cr-0,2-1=0.00460 M, Cr3+1=1.0x102 M. The Nerst equation is E=E - (0.0592/n)logQ
help with this one
Construct a galvanic cell using the following half-reactions: Cr3+ (aq) + 3e - Cr(s) º = -0.56 V 2 Hg2+(aq) + 2e - H922+(aq) = 0.92 V 2 Ho2+ The initial concentrations are: [Cr3+] =0.31 M [Hg2+] =2.57 M [Hg22+] =0.49 M (1) What is the potential of this non-standard cell at 298 K? Give your answer to 3 sig. figs. E(V) = Submit Answer Tries 0/2 (ii) How will each of the following changes to...
Consider the galvanic cell that uses the reaction 2 Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + 2 Ag (s) Clearly sketch the experimental set-up, write down the anode and cathode half-reactions, and give the shorthand notation for the cell.
7. A is cell made by placing Zn(s) in Zn2 (aq) and Au(s) in Au (aq). Use Standard Reduction Potentials. (12 points) a. Write the half reaction for the reaction at the cathode: Calculate the voltage for the standard cell (IM Zn2* (aq) and 1 M Au?* (aq). c. Calculate the voltage for the cell after it is 999% used up. Assume 1.00 L of each solution. (Hint: Write the overall equation.)
A galvanic cell is based on the following half reactions E° (V) Au33e Au 1.50 Mg22e Mg -2.37 Calculate the standard potential for this cell V This cell is set up at 25°C with [Mg2 ]= 1.00 x 10-M The cell potential is observed to be 3.97 V. Calculate the [Au3*] that must be present (Enter your answer to three significant figures.) [Au3 Submit Hide Hints Hint 2 Hint 1 Hint 3 Write the Nernst equation for the cell reaction....
cell A voltaic cell employs the following redox reaction: Cu(s) + 2 Ag+ (aq) – Cu 2+ (aq) + 2 Ag(s) The E° for the reaction is +0.46 V. The initial (nonstandard) conditions are: [Ag +] = 0.025M; [Cu 2+] = 2.0 M Part a. Write the half-reaction that occurs at the anode. Part b. Write the half-reaction that occurs at the cathode. Part c. How many electrons are transferred in this reaction? Part d. What is the cell potential,...