Calculate the mass of Al that is produced during a one hour electrolysis on AlCl3 if the current is 3 ampere.
Calculate the mass of Al that is produced during a one hour electrolysis on AlCl3 if...
Calculate mass of Al formed by electrolysis of molten AlCl3 by a current 7.5*10^4 A flowing for period 45h.
um CollUl exceed 100%. Calculate the grams of aluminum metal produced from the electrolysis one hr with an electrical current of 15.0 amperes. al produced from the electrolysis of molten AlCl3 for 3.25 electrical current of 15.0 amperes. Work must be shown to receive credit. 6 points
what mass of silver (Ag) metal can be produced in 1 hour in the electrolysis of Ag+ salt by a current of 12 A?
What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by a current of 26 A? Express your answer using two significant figures.
What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt by a current of 23 A?! Express your answer using two significant figures. 140 AEDROO? Submit Request Answer
3. Determine the limiting reactant and the mass of AlCl3 produced by reacting 15.0 g of Al with 30.0 g of Cly according to the following chemical equation. The molar mass of AICI is 133.33 g/mol. A1 = 26.98 g/mol 2 Al(s) + 3 Cl2 (g) → 2 AlCl3(s) C1 = 35.45 g/mol A) Al is the limiting reactant, 32.4 g of AlCl3 produced. B) Al is the limiting reactant, 74.1 g of AlCl3 produced. C) Cl2 is the limiting...
Calculate the mass of nickel produced in 1.00 hr by the electrolysis of aqueous NiCl2 if the electrical current is 18.0 A.
11. Calculate the volume of oxygen produced (measured at s,t,p) during electrolysis of sodium sulfate solution if you use of current 0.50 amp for 30 min
Calculate the number of grams of copper produced in 5.67 hours by the electrolysis of molten CuCl2 if the electrical current is 11.7 A. You may assume the molar mass of elemental copper is 63.546 g/mol.
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...