Al3+(aq) +3e = Al(s)-1.67VFe2+(aq) + 2e = Fe(s)-0.44VCalculate the cell voltage for the cell belowAl(s) | A³ (0.18M) || Fe2+ (0.85M) | Fe(s)Insert your response as a numerical value to 2 decimal places. Include a sign. Do NOT includea space between the sign and the value. DO NOT include units. e.g. -0.21

Step 1: Recall that in an electrochemical cell, oxidation occurs in the anode and reduction occurs…

Answered: Al3+(aq) +3e = Al(s) -1.67V Fe2+(aq) +…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 50QRT

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Similar questions

Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
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What is the cell potential (Ecell) of a spontaneous cell that is run at 25C and contains [Cr3+] = 0.10 M and [Ag+] = 1.0 104 M?
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The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
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Consider a cell in which the reaction is 2Ag(s)+Cu2+(aq)2Ag+(aq)+Cu(s) (a) Calculate E° for this cell. (b) Chloride ions are added to the Ag|Ag+ half-cell to precipitate AgCl. The measured voltage is +0.060 V. Taking [Cu2+]=1.0M, calculate [Ag+]. (c) Taking [Cl-] in (b) to be 0.10 M, calculate Kspof AgCl.
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Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.

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