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) 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
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
A voltaic cell is constructed using silver and aluminum. The following is the unbalanced redox reaction: Ag+ (aq) + Al(s) Ag (s) + A13+ (aq) What is the correct, balanced redox reaction that occurs in the cell? O A 5 Ag+ (aq) + 3 AI (5) - 5 Ag (s) + 3 A13+ (aq) O B. Ag* (aq) + 4 AI (5) ► Ag (s) + 4 A13+ (aq) OC 3 Ag* (aq) + Al(s) — 3 Ag (s) +...
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...
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....
a) Which statement is true for an electrolytic cell? O a. It produces electrical current from electricity. O b. It consumes electrical current to drive a spontaneous chemical reaction. O c. It produces electrical current from a spontaneous chemical reaction. Od. It consumes electrical current to drive a nonspontaneous chemical reaction. b) Balance the following redox reaction in acidic solution. What are the coefficients in front of Al(s) and H2O in the balanced reaction? MnO 4 (aq) + Al(s) +...
How many minutes will it take to plate out 16.22 g of Al metal from a solution of A13+ using a current of 14.6 amps in an electrolytic cell? A) 53.0 B) 66.2 C) 153 D) 199 E) 11900