30 escA galvanic cell is set up with iron and aluminum half-cells, according to the unbalanced reaction below. If the concentration of Fe2+ is 0.0011 M and theconcentration of A13+ is 0.77 M, what is the Ecell in volts?Fe2+ (aq) + Al(s) → Fe(s) + Al³+ (aq)E cell = +1.22 VO A. 0.00 VOB. 1.23 VOC. 0.964 VOD. 1.13 VOE. 1.39 VOF. 1.20 VO G. 1.33 VOH. 1.05 VOI. 1.28 VOJ. 1.22 V<< Question 30 of 32 > >>Moving to another question will save this response.MacBook AirF123²FR8.0Fo!1A2F2WS#3F3EDC$4F4RF%5VF5TG< 6YB&7HF7UN*008JDIIFBI(9MF9KOOF10P;..[I

We can calculate Ecell by using Nerst equation

A galvanic cell is set up with iron and aluminum half-cells, according to the unbalanced reaction below. If the concentration of Fe2+ is 0.0011 M and the concentration of A13+ is 0.77 M, what is the Ecell in volts? Fe2+ (aq) + Al(s) → Fe(s) + A1³+ (aq) E cell = +1.22 V OA. 0.00 V OB. 1.23 V OC. 0.964 V OD. 1.13 V OE. 1.39 V OF. 1.20 V OG. 1.33 V OH. 1.05 V OL 1.28 V OJ. 1.22 V

A galvanic cell is set up with iron and aluminum half-cells, according to the unbalanced reaction below. If the concentration of Fe2+ is 0.0011 M and the concentration of A13+ is 0.77 M, what is the Ecell in volts? Fe2+ (aq) + Al(s) → Fe(s) + A1³+ (aq) E cell = +1.22 V OA. 0.00 V OB. 1.23 V OC. 0.964 V OD. 1.13 V OE. 1.39 V OF. 1.20 V OG. 1.33 V OH. 1.05 V OL 1.28 V OJ. 1.22 V

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 135CWP: Consider a galvanic cell based on the following half-reactions: a. What is the expected cell...

See similar textbooks

Similar questions

Consider a galvanic cell based on the following half-reactions: a. What is the expected cell potential with all components in their standard states? b. What is the oxidizing agent in the overall cell reaction? c. What substances make up the anode compartment? d. In the standard cell, in which direction do the electrons flow? e. How many electrons are transferred per unit of cell reaction? f. If this cell is set up at 25C with [Fe2+] = 2.00 104 M and [La3+] = 3.00 103 M, what is the expected cell potential?
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [MnO4] = 0.010 M, [Br] = 0.010 M. [Mn2] = 0.15 M, and [H] = 1.0 M. 2MNO4(aq)+10Br(aq)+16H+(aq)2MN2(aq)+5Br2(l)+8H2O(l)
Given this reaction, its standard potential, and the standard half-cell potential of 0.34 V for the Cu2+ |Cu half-cell, calculate E° for the Fe(s)|Fe2+(aq) half-cell.
What is the standard cell potential you would obtain from a cell at 25C using an electrode in which Hg22+(aq) is in contact with mercury metal and an electrode in which an aluminum strip dips into a solution of Al3+(aq)?
Calculate the cell potential of a cell operating with the following reaction at 25C, in which [Cr2O32] = 0.020 M, [I] = 0.015 M, [Cr3+] = 0.40 M, and [H+] = 0.60 M. Cr2O72(aq)+6I(aq)+14H+(aq)2Cr3+(aq)+3I2(s)+7H2O(l)
For each reaction listed, determine its standard cell potential at 25 C and whether the reaction is spontaneous at standard conditions. (a) Mn(s)+Ni2+(aq)Mn2+(aq)+Ni(s) (b) 3Cu2+(aq)+2Al(s)2Al3+(aq)+3Cu(s) (c) Na(s)+LiNO3(aq)NaNO3(aq)+Li(s) (d) Ca(NO3)2(aq)+Ba(s)Ba(NO3)2(aq)+Ca(s)
An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
Which of the changes below will increase the voltage of the following cell? Co|Co2+(0.010M)H+(0.010M)|H2(0.500atm)|Pt (a) Increase the volume of COCl2 solution from 100 mL to 300 mL. (b) Increase [H+] from 0.010 M to 0.500 M. (c) Increase the pressure of H2 from 0.500 atm to 1 atm. (d) Increase the mass of the Co electrode from 15 g to 25 g. (e) Increase [CO2+] from 0.010 M to 0.500 M.