ELECTROCHEMISTRY: Copper was electroplated from a Cuzs04 solution onto an electrode with an active surface area of 6 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 4.34 A for 0.7772 hours. (density of Cu 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)

ELECTROCHEMISTRY: Copper was electroplated from a Cuzs04 solution onto an electrode with an active surface area of 6 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 4.34 A for 0.7772 hours. (density of Cu 8.96 g/cm3, MW of Cu = 63.55 g/mol). (Input values only with 2 decimal places. Do not include the unit.)

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 Na + concentration of a solution was determined by measurements performed with a sodium ion selective electrode. The electrode system has developed a potential for - 0.2831 V when immersed in 15.00 mL of the solution of unknown concentration. After adding 5.00 mL of NaCℓ 1.00 x 10-2 mol / L to the solution of unknown concentration, the potential went to -0.1546 V. Calculate the Na + concentration in the original solution.
Cd + Pb2+ <-> Cd2+ + Pb Pb: ΔHfo = ΔGfo = 0 kJ/mol. ΔSfo = 68.85 J/mol-K. Calculate the ΔG (in kJ) if the potential, E, of the cell was measured as +0.29V.
2. One of the most problems encountered. Molecular masses can be determined through electroplating. Determine the molecular mass and identity of a +2 metal, X, that plates 46.3g of X in 6.75 hours at a current of 2 A.
copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of 6.8 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 4.68 A for 1.3998 hours. (density of Cu = 8.96 g/cm3, MW of Cu = 63.55 g/mol).
The reduction potential to the metal of Ba 2+ is -1.57 V and that of Cu 2+ is +0.34 V. The cell potential for the reaction Ba(s) + Cu 2+ (aq) → Ba 2+ (aq) + Cu(s) is therefore: a. (+1.57) + (+0.34) b. (+1.57) + (-0.34) c. (-1.57) + (+0.34) d. 2 x (-1.57) + 2 x (0.34) e. (-1.57) + (0.34)
Write the line notation for the following cell. Pt HBr(aq, 0.10 M) Line notation: Br₂(/) AI(NO3)3(aq, 0.010 M) Al AI(NO3)3(aq, 0.010 M) Answer Bank HBr(aq, 0.10 M) Pt(s) Al(s) Br₂ (1)
Copper was electroplated from a Cu2SO4 solution onto an electrode with an active surface area of 3.25 cm2. Determine the thickness (mm) of the deposit if the current is kept constant at 4.06 A for 0.9497 hours.
Calculate the required voltage (V) if an unknown metal (M) was electrodeposited from an aqueous solution containing M2X1 (where X is the anion) with a supplied current of 4.98 A for 11 h, consuming 0.1145 kWh of electrical energy. Assume that the current efficiency is 93%. (Input values only with 2 decimal places
A solution containing Pt4t is electrolyzed with a current of 4.30 A. How long will it take to plate out 99% of the platinum in 0.55 L of a 0.030-M solution of Pt4+? Time =
Calculate the AG for the cell: Cu(s)|Cu*2 (0.010 M)|| Ag*(0.050 M)|Ag(s). E°Cu| Cu+2 = 0.337 V Ag | Ag+ = 0.799 V -85.7 kJ -87.4 kJ -89.2 kJ -92.6 kJ
What mass of platinum can be played onto an electrode dipped in Pt(NO3)2 solution if a 2.5 current is applied for 4.0 hours?