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
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20;. The cell potential of the following electrochemical cell depends on the gold concentration in the...
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 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
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
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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
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures. H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq) The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. Pt(s) l Cr3+(aq),...