Exercise 19.106 Part A The cell potential of the following electrochemical cell depends on the gold...
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt($)|H2(9, 1.0 bar) H+ (aq, 1.0 mol L-Aus+ (aq,? mol L-)|Au(s). Part A What is the concentration of Au3+ in the solution if Ecell is 1.23 V ? Express your answer using two significant figures. YO ALC * * O O ? Au3+1 = mol L-1 Submit Request Answer
20;. The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt(s) | H2(g,1atm) | H+(aq,1.0M) | Au3+(aq,?M) | Au(s). What is the concentration of Au3+ in the solution if Ecell is 1.22 V ? Express your answer using two significant figures. [Au3+] = ______ M
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt(s)|H2(g,1atm)|H+(aq,1.0M)|Au3+(aq,?M)|Au(s). What is the concentration of Au3+ in the solution if Ecell is 1.257 V ? Express your answer using three significant figures and in fM (f = femto = 10-15).
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt(s)|H2(g,1atm)|H+(aq,1.0M)||Au3+(aq,?M)|Au(s). What is the concentration of Au3+ in the solution if Ecell is 1.26 V ? To what pH should you adjust a standard hydrogen electrode to get an electrode potential of -0.117 V ? (Assume that the partial pressure of hydrogen gas remains at 1 atm.) Express your answer using two decimal places.
The cell potential of the following electrochemical cell depends on the pH of the solution in the anode half-cell: Pt(s)|H2(g,1atm)|H+(aq,?M)||Cu2+(aq,1.0M)|Cu(s). What is the pH of the solution if Ecell is 360 mV ?
MISSED THIS? Read Section 20.6 (Page) An electrochemical cell is based on the following two half-reactions: Part A oxidation: Sn (s) +Sn2+ (aq, 1.80 M )+2e reduction: C1O2(g, 0.210 atm )+e- +C10] (aq, 1.70 M) Compute the cell potential at 25°C. Express the cell potential to three significant figures. ΤΕΙ ΑΣφ ? Ecell = .839 Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining Provide Feedback
A. Calculate the cell potential that would result in the following electrochemical cell at 25oC: Pt | UO22+(0.10M),U4+(0.22M),H+(0.60M) || Ag+(0.034M) | Ag Line notation is anode || cathode Write Nernst equations for the anode and cathode separately. Then Ecell = Ecathode - E anode B. If the electrochemical cell Ag/AgCl || Zn2+(x M) | Zn(s) develops a potential of -1.039 volts at 25oC, what is the Zn2+ concentration in the solution? (Answer in decimal format) Ag/AgCl reference electrode has E=0.199...
3. Consider the following electrochemical cell. Standard reduction potentials are given on the next page. Tl(s) | Tl+(aq, 0.50 mol L−1) || H+(aq, x mol L−1) | H2(g, 1 atm) | Pt(s) The concentration of H+ is unknown and the pressure of H2 is kept constant at 1 atm. The cell voltage is initially measured as 0.139 V, with the Pt | H2 | H+ half-cell acting as the cathode. (a) (6 marks) Write out the oxidation and reduction half...
calculate ecell for the following electrochemical cell at 25 C. Pt(s)| H2 (g,1.00 atm) | H+ (aq, 1.00 M) || (Pb2+ (aq, 0.150 M) | Pb (s) Pb^2+(aq) + 2e- ---> Pb (s) Eo=-0.126 V 2H^+ (aq) + 2e- ---> H2 (g) Eo=0.00 V Thank you!
A. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 7.45×10-4 atm, the Cl- concentration is 1.21M, and the Cr3+ concentration is 1.37M ? 3Cl2(g) + 2Cr(s)6Cl-(aq) + 2Cr3+(aq) Answer: _____ V The cell reaction as written above is spontaneous for the concentrations given: ____ (true/false) B. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following...