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...
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 1.26 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 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
Exercise 19.106 Part A The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half-cell: Pt(s) H2 (9,1 atm) H+(aq, 1.0 M) Au'+(aq, ?M) Au(s). What is the concentration of Au”+ in the solution if Ecell is 1.24 V? Express your answer using two significant figures. O AIO O O ? [Aud+] = Submit Previous Answers Request Answer X Incorrect; Try Again
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 ?
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)||Cu^2+(aq,1.0M)|Cu(s)what is the pH of the solution if Ecell is 375 mV
An electrochemical cell involves the Au3+/Au and the acidic MnO4-/Mn2+ half-cells. For standard conditions, the anode is the gold cell. Calculate the pH (to two decimal places) required to make the gold cell the cathode. Assume an Ecell of 0.01 V. E (Au +) = 1.42V E (8H+ +MnO4-) = 1.55V
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...
For the electrochemical cell below, the half-cell on the left is the anode and the cell potential is 0.183 V at 25 °C. What is the concentration of H+, x, in mol L-1? Note: The symbol M is an abbreviation for mol L-1. Pt(s) | V2*(aq, 0.620 M), va(aq, 0.650 M) || H'(aq, xM) | H2(g, 1.30 bar) Pt(s) Half reaction 2 H(aq) 2eH2(g) V(a)V(aq) Eo V 0.000 -0.255 Enter a value accurate to 3 significant figures. x-[H]Number mol L-1
The following electrochemical cell was constructed with an unknown concentration of Cl- in the cathode. S.H.E || Cl- (aq, x M) | AgCl (s) | Ag(s) a. write the overall cell reaction b. If the cell potential at 25 C was measured to be +0.267 V, what is the molarity of Cl- in the cathode compartment?