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.
1. Determine the mass (g) of aluminum deposited in an electrolytic cell using a current of...
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
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
correct answer? The change in Gibbs free energy, AGⓇ for the following reaction at 298 K is 70.6 kJ/mol. 2NO,(9) — 2NO(g) + O2(9) What is Keq for this reaction? O 4.30 O 0.971 2.00 1.03 O 0.936
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...
Question 1 Prior to 1886, Aluminum was rarer and more expensive than gold! It was in 1886, that brother and sister Charles Martin Hall and Julia Brainerd Hall discovered the electrolytic process that separated Aluminum from Aluminum Oxide ore. Today, over 41 million tons are processed for use in everything from beer cans to aircraft skins. a) How many coulombs of electricity must pass through the cell to produce 40.0 g of Aluminum (26.981539 g/mol)Fm an Ala(Soy), cap solution "....