レQuestion 17 of 20へGeneral Chemistry 4th EditionUniversity Sciepresented by MaMcQuarrie Rock GalloglyThe voltage generated by the zinc concentration cell described by the line notationZn(s) Zn*(aq, 0.100 M) || Zn2+(aq, ? M) | Zn(s)is 15.0 mV at 25 °C. Calculate the concentration of the Zn+(aq) ion at the cathode.concentration:Question Source: McQuarrie, Rock, And Gallogly 4e - General ChemsitryPublisi

Lower the value of standard reduction potential, then the given electrode acts as anode and higher the value of standard reduction potential, then the given electrode acts as cathode. a. The anode half reaction (oxidation): Zn(s) --> Zn2+(aq)+ 2e- The cathode half reaction (reduction): Zn2+(aq)+ 2e- - --> Zn(s) The overall cell reaction : Zn(s) + Zn2+(aq, xM) --------> Zn2+(aq, 0.100 M) +Zn(s) E0cell = E0 cathode - E0 anode = -0.74-(-0.74) = 0.0 V Also given emf of the cell, Ecell = 15.0 mV = 15.0 ×10-3 V The cell potential of the cell at 25 degree Celsius at different condition is given by Nernst equation Ecell = E0 cell- (0.05912)log([Zn2+]anode[Zn2+]cathode) 15.0 ×10-3 = 0.0 - (0.05912)log(0.100[Zn2+]cathode) 30.0 ×10-3 = - (0.0591)log(0.100[Zn2+]cathode) [Zn2+]cathode = 0.3218 M Result: The concentration of the Zn2+ion at the cathode = 0.3218 M

Science

Chemistry

General Chemistry 4th Edition McQuarrie • Rock Gallogly University Sci presented by M The voltage generated by the zinc concentration cell described by the line notation Zn(s) Zn+(aq. 0.100 M) Zn²+(aq, ? M) Zn(s) is 15.0 mV at 25 °C. Calculate the concentration of the Zn+(aq) ion at the cathode. concentration:

General Chemistry 4th Edition McQuarrie • Rock Gallogly University Sci presented by M The voltage generated by the zinc concentration cell described by the line notation Zn(s) Zn+(aq. 0.100 M) Zn²+(aq, ? M) Zn(s) is 15.0 mV at 25 °C. Calculate the concentration of the Zn+(aq) ion at the cathode. concentration:

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Assume a concentration cell with a zinc anode and a zinc cathode. The anode is surrounded by a 100 ml ZnSO4 solution of 0.01 mol/l concentration. The cathode is surrounded by a 100 ml ZnSO4 solution with a concnetration of 1 mol/l. A salt bridge ensures neutrality of both solutions during the reaction. This system can be described in short-hand notation as: Zn(s) | Zn²+ (aq) (0.01 M) II Zn²+ (aq) (1 M) I Zn(s) The temperature is 25°C. Part D Determine the initial voltage of this concentration cell. Provide your result with three significant figures in the appropriate units. AE 59.2 mV Submit Previous Answers Correct
Use the standard half-cell potentials Click to open: to calculate the standard cell potential (Eºcell) and the standard free energy (AGO) for the following reaction. • Answer: Eºcell = [Select] . Answer: AG° = [Select] Co(s) + F2(g) → Co2+ (aq) + 2F (aq) V kJ
The voltage generated by the zinc concentration cell described by the line notation Zn(s) | Zn2+(aq,0.100 M) ‖ Zn2+(aq,? M) | Zn(s) is 18.0 mV at 25 °C. Calculate the concentration of the Zn2+(aq) ion at the cathode.
A current of 250. A flows for 24.0 hours at an anode where the reaction occurring is as follows: Mn2+ (aq) + 2H₂O(1) MnO2 (s) + 4H(aq) + 2e What mass of MnO2 is deposited at this anode?
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.96 minutes for a current of 1.62 A to plate 0.0534 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.62 minutes for a current of 1.79 A to plate 0.0731 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
A current of 8.86×104 A is passed through an electrolysis cell containing molten KCl for 12.7 days.(a) How many grams of potassium are produced? _________g(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? _________L
Consider the following electrochemical cell at 298 K where the source of Cu2+ (aq) is the sparingly soluble salt CuX. Zn(s)|Zn²* (aq, 0.50M)||Cu²+ (aq)|Cu(s) Zn2* + 2e = Zn E° = -0.76 V Cu2+ + 2e = Cu E° = 0.34 V If the potential created from this cell = 1.03 V, what is Ksp for CuX? O 1.9x10-9 3.8x10 12 4.6x10 6 2.0x10 7
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.41 minutes for a current of 1.38 A to plate 0.0572 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
Enter electrons as e A voltaic cell is constructed in which the anode is a Fe2+|Fe3+ half cell and the cathode is a F|F, half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: +. In the external circuit, electrons migrate the Fe2+|Fe3+ electrode the F|F, electrode. from to In the salt bridge, anions migrate the F|F, compartment 3- the Fe2+|Fe+ compartment. +. +. 1
ELECTROCHEMISTRY: Determine the molar mass (amu) of Metal (M) if it took 1.24 minutes for a current of 1.75 A to plate 0.0893 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not inciude the unit.)
The potential, AE°, for an electrochemical cell for the reaction shown below is 0.339 V: Cu2*(aq) + H2(g) = Cu(s) + 2H*(aq) (1) What is AE° for reaction 2? ½Cu2*(aq) + ½H2(g) = ½Cu(s) + H*(aq) (2) Select your response from the list below. i) 0.339 V ii) 0.678 V iii) 0.1695 V