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? |
Enter your answer in the provided box. A constant current is passed through an electrolytic cell...
please help me! Enter your answer in the provided box. A constant current is passed through an electrolytic cell containing molten MgCl2 for 15.0 h. If 8.70 x 109 g of Cl, are obtained, what is the current in amperes?
5 attempts left Check my work Enter your answer in the provided box. A constant current is passed through an electrolytic cell containing molten MgC2 for 17.0 h. If 4.30 x 105 g of Cl2 are obtained, what is the current in amperes?
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
How long (hr) must a constant current of 50.0 A be passed through an electrolytic cell containing Color copper metal? Enter your answer with two decimal places and no units. How long (hr) must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Caders to produce 100 copper metal? Enter your answer with two decimal places and no units.
Enter your answer in the provided box. How many grams of aluminum can form by passing 347 C through an electrolytic cell containing a molten aluminum salt?
How long must a constant current of 50.0 A be passed through an electrolytic cell containing aqueous Culons to produce 400 moles of copper metal? 0.466 hours 429 hours 2. 14 hours 0.233 hours O
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.
Enter your answer in the provided box. A current of 0.150 copper deposited. A passed for 16.0 min through a CuSO4 solution. Calculate the amount of
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...
what are 17 and 18? Question 17 (10 points) A constant current is passed through a solution of Agt in an electrolytic cell. In 3.0 minutes, 0.65 g of silver is deposited at the cathode. The number of moles of electrons passed into the Agt solution is mole. (Please enter your answer in decimal form, such as 0.021, and keep 2 significant figures.) The total coulombs of charge passed into the Cu2+ solution is C. (Please enter your answer in...