A current of 3.00 amperes is passed through molten MgBr2 for 1.00 hour. The masses, in...
3. A steady electric current is passed through molten MgCl, for exactly 1.00 hour, producing 243 grams of Mg metal. If the same current is passed through molten AICI, for 1.00 hour, what is the mass of Al metal produced?
A current of 0.42A is passed through a similar electrolytic cell set-up containing molten CaCl2 for 2.2 hours. Calcium metal is deposited at the cathode, and chlorine gas is generated and collected at the anode. Write the electrode reactions and calculate the amount of calcium metal (in grams) formed as well as the pressure of chlorine gas (in atm). Assume 330mL of gas was collected at 273K.
A current of 7.49×104 A is passed through an electrolysis cell containing molten NaCl for 9.40 days. (a) How many grams of sodium are produced? g (b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? L
A current of 7.11x104 A is passed through an electrolysis cell containing molten NaCl for 6.30 days. (a) How many grams of sodium are produced? (b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm? L
Molten salts When electricity is applied to a molten binary salt, the cation will be reduced and the anion will be oxidized. The electrolysis of CaBrz (), for example, produces Ca(s) at the cathode (from the reduction of Ca2+) and Br2(1) at the anode (from the oxidation of Br"). If more than one cation is present, only the one with highest reduction potential will be reduced. Similarly, if more than one anion is present, only the one with the highest...
Current is applied to a molten mixture of CuF, ZnCl2, and Mgl2. Standard potentials may be found here. Select the chemical species produced at the cathode. Select the chemical species produced at the anode O Cl2 O Cu O Cl2 O Zn 12 O 12 O F2 O Mg O Cu O F2
A current of 0.50 amperes flowed through a cell for two hours in which CuSO_4 is the electrolyte. a. Write the anode reaction for the cell. b. How many Coulombs of electricity are generated? c. How many Faradays arc generated? d. How many moles of electrons arc generated? e. Calculate the change in mass of the cathode of this cell.
Question 16 (5 points) A constant current of 0.912 A is passed through an electrolytic cell containing molten MgCl2 for 7.25 h. What mass of Mg is produced? Faraday constant, 95485 C mol-1 Molar mass Mg 24.31 g/mol MgCl2 95.21 g/mol
9. In the electrolysis of molten MgCh2. A current of 60.0 A passes through molten MgCl; for a period 2 h. Calculate the mass in grams of Mg (AM: 24.3) produced. (F 96485 C/mol e) [10 pt]
Enter your answer in the provided box. A constant current is passed through an electrolytic cell containing molten MgCl2 for 13.0 h. If 9.80 ×105 g of Cl2 are obtained, what is the current in amperes?