Determine the mass (g) of aluminum deposited in an electrolytic cell using a current of 0.750 A for 1.2 hour (1 hour = 3,600 s)
Al3+(aq) + 3e- ⟶ Al(s)
A. 0.000839 g
B. 2.20 g
C. 0.302 g
D. 0.625 g
E. 0.906 g
Determine the mass (g) of aluminum deposited in an electrolytic cell using a current of 0.750...
Determine the mass (g) of aluminum deposited in an electrolytic cell using a current of 0.750 A for 1.2 hour (1 hour = 3,600 s) Al3+ (aq) + 3e - Al(s) 0.302 g 0.000839 g 0.625 g 0.906 g O 2.20 g
Determine the mass (g) of aluminum deposited in an electrolytic cell using a current of 0.750 A for 1.2 hour (1 hour = 3,600 s) A13+ (aq) + 3e - Al(s) O 0.000839 g 0 2.20 g 0 0.3029 O 0.906 g O 0.625 g
1. Determine the mass (g) of aluminum deposited in an electrolytic cell using a current of 0.750 A for 1.2 hour (1 hour = 3,600 s) Al3+(aq) + 3e- ⟶ Al(s) 0.302 g 0.000839 g 0.625 g 0.906 g 2.20 g 2. The change in Gibbs free energy, ∆G°, for the following reaction at 298 K is 70.6 kJ/mol. 2NO₂(g) ⟶ 2NO(g) + O₂(g) What is Keqfor this reaction? 1.03 0.971 4.30 2.00 0.936 3.
What mass of silver is deposited on the cathode of an electrolytic cell if an electric current of 2.86 A is run through a solution of AgNO3 for one hour? Select one: O a. 11.5 g O b. 5.76 g O c. Og O d. 0.11 g o e. 0.192 g
Given the following electrolytic cell: The current is discharged into the electrolytic cell containing the solution CuSO4(aq) 1.0M at 25 oC. During the operation of the cell, copper Cu(s) is deposited on one electrode and oxygen O2(g) gas is released, near the second electrode. O2(g) + 4H3O+(aq) + 4e- 6H2O(l) Eo= 1.23V Cu2+(aq) + 2e- Cu(s) Eo= 0.34V A. Write the direction of the flow of electrons in the cell. B. Write the electrolysis equation that occurs in the cell....
Calculate E°cell for a silver-aluminum cell in which the cell reaction is?Al(s) + 3Ag+(aq) ? Al3+(aq) + 3Ag(s)A. -2.46 V B. 0.86 V C. -0.86 V D. 2.46 V E. none of these
Given the following electrolytic cell: The current is discharged into the electrolytic cell containing the solution CuSO4(aq) 1.0M at 25 oC. During the operation of the cell, copper Cu(s) is deposited on one electrode and oxygen O2(g) gas is released, near the second electrode. O2(g) + 4H3O+(aq) + 4e- 6H2O(l) Eo= 1.23V Cu2+(aq) + 2e- Cu(s) Eo= 0.34V A. The current in the cell is 1.5 amperes. The current is streamed in 40 minutes. i. Calculate the mass of copper...
electrolytic cell 6A Practical Application of the electrolysis process. How much does it cost to generate the mass of aluminum (14.0 g) in one beverage can The aluminum in the can is produced by reducing Al+ to Al(s). The reaction is run commercially at 50,000 A and 4.0 V (4.0 J/C), 1 kWh ofelectricity cost about 10 cents and 1 kWh is 3.60 x 10s J. Energy charge x voltage. 6A Practical Application of the electrolysis process. How much does...
Two electrolytic cells are connected in series and the same current flows through both. In one cell Ag+ ions are reduced to Ag(s); in the other cell Cr6+ ions are reduced to Cr(s). If 100 g of silver metal are plated out in the silver cell, what mass, in g, of Cr(s) will be deposited in the other cell? A. 48.2 B. 207 C. 4.0 D.16.1 E.8.0
Please explain what you do and why. A galvanic cell is setup with the following two half-cells: A 250.0 mL solution of 0.15 M aluminum nitrate with a platinum electrode. A 250.0 mL solution of 0.85 M cobalt(II) nitrate with a cobalt electrode. a) Determine the cell potential that will be initially measured for this galvanic cell b) How much mass is gained/lost by the cobalt electrode after the cell reaches equilibrium? c) If it takes this galvanic cell 2.00...