A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at 25.0°C and each compartment has a volume of 219 mL. The cell delivers 0.25 A for 31.5 h. (a) How many grams of Cu are deposited? 4) 9.3 (b) What is the [Mg2+ ]? Assume constant volumes. 40.66826 X mol·L-1

A galvanic cell using Mg|Mg2+ and Cu|Cu2+ half-cells operates under standard-state conditions at 25.0°C and each compartment has a volume of 219 mL. The cell delivers 0.25 A for 31.5 h. (a) How many grams of Cu are deposited? 4) 9.3 (b) What is the [Mg2+ ]? Assume constant volumes. 40.66826 X mol·L-1

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

The potential of a cell under standard conditions can be calculated as: (a) The algebraic sum of the normal oxidation potentials of the anode and cathode (b) The sum of the normal oxidation potential of the anode and the normal reduction potential of the cathode (c) The difference between the normal reduction potential of the anode and the normal reduction potential of the cathode (d) The difference between the normal reduction potential of the cathode and the normal reduction potential of the anode
3.2 calculate the standard cell potential of the following cell at 25C Sn(s)|Sn"(aq)||Cu?²*(aq)|Cu(s)
2. (a) A voltaic cell is constructed as follows: Zn | Zn²+ | H*|H₂ The half-cell reactions are: Zn →Zn²+ze E = 0.76 V If the voltage of the cell is 0.45V at 25°C when [Zn²] = 1.0 M and PH₂ = 1.0 atm, what is [H+]? 2H+ + 2e- → H₂ EⓇ = 0.0V (b) For the voltaic cell described in part (a), find the pH of the cathodic solution when pH2 = 1.0 atm and [Zn²+]= 0.1 M and the E*cell = 0.542 V. (c) What amount of time is needed to plate 2.08 g of copper at a constant current flow of 1.26 A from a 0.1 M CUSO4 solution? Cu²+ +ze--- Cu(s)
Qq.49. Subject :- Chemistry
Predict the half-reaction occurring at the anode and the half-reaction occurring at the cathode for electrolysis for each reaction.(a) a mixture of molten AlBr3 and MgBr2(b) an aqueous solution of LiI
I need help with all parts. Thanks
The following figure represents an electrochemical cell at 25.00C with aqueous solutions that behave ideally: (a) Represent the electrochemical cell using cell notation, by taking into account that concentrations of the ZnSO4 and CuSO4 solutions are 0.25 M and 0.35 M, respectively. (b) Calculate the standard potential of the cell, E0cell. (c) Calculate the potential of the cell, Ecell. (d)Calculate DG0 (e)Calculate DG (f)Calculate the equilibrium constant, K.
(19) sa len Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu²+ (aq) → Cr³+ (aq) + Cu+ (aq) If the cell is operating at 25°C, what is the value of the equilibrium constant (Kea)? (A) 1.41 x 10¹¹ (B) 1.19 x 1018 (C) 5.53 x 105 (D) 2.79 x 1033 (E) 1.81 x 10-6 11020 ucleus of calcium-39 captures one
A galvanic cell is prepared according to the redox reaction shown below. A voltmeter connected to this galvanic cell under standard conditions reads 0.45 V, and AG, xn = -79 kJ/mol. If the concentration of Fe2+ is increased to 2.0 M, then Ecell will and AGrxn will be than AGxn- Fe(s) + 2H*(aq) Fe2* + H2(g) decrease, less negative O decrease, more negative O increase, more negative O increase, less negative
A galvanic cell is constructed in which the overall reac- tion is Pb(s) + 2 H;O* (aq) → Pb²+ (aq) + H2 (g) + 2 H20(e) (a) Calculate AE° for this cell. (b) Chloride ions are added until PbCl, precipitates at the anode and [CI-] reaches 0.15 M. The cell potential is then measured to be 0.22 V at pH = 0 and PH, 1.0 atm. Calculate [Pb2+] under these conditions. (c) Calculate the solubility product constant Kp of PbCl2.
(19) Consider the following redox reaction that occurs in a voltaic cell: Cr2+ (aq) + Cu²+ (aq) → Cr³+ (aq) + Cut (aq) If the cell is operating at 25°C, what is the value of the equilibrium constant (Keq)? (A) 1.41 x 10¹1 1.19 x 1018 5.53 x 105 2.79 x 1033 1.81 x 10-6 (B) (C) (D) (E)
Help with the following question Please round the answer to 3 sig figs