what are 17 and 18? Question 17 (10 points) A constant current is passed through a...
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Question 17 (10 points) Saved A constant current is passed through a solution of Cu2+ in an electrolytic cell. In 3.5 minutes, 0.21 g of copper is deposited at the cathode. The number of moles of electrons passed into the Cu2+ solution is 0.0066 mole. (Please enter your answer in decimal form, such as 0.021, and keep 2 significant...
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.
When electricity (the flow of electrons) is passed through a solution, it causes an oxidation-reduction (redox) reaction to occur. If the solution contains a metal cation such as Ag+, the flow of electrons will reduce the silver ion, causing solid silver to plate onto the electrode. The amount of metal plated depends on the number of electrons passed. The total charge of a mole of electrons is 96,485 coulombs (C) and 1 ampere (A) = 1 coulomb/second (C/s) Part A...
Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive) layer of a precious metal, such as silver or gold. In essence the metal object is made the cathode of an electrolytic cell in which the precious metal cations are dissolved in aqueous solution. Suppose a current of 300.mA is passed through an electroplating cell with an aqueous solution of Ag2SO4 in the cathode compartment for 55.0 seconds. Calculate the mass of pure...
Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive) layer of a precious metal, such as silver or gold. In essence the metal object is made the cathode of an electrolytic cell in which the precious metal cations are dissolved in aqueous solution. Suppose a current of 0.310 A is passed through an electroplating cell with an aqueous solution of Ag2SO4 in the cathode compartment for 54.0 seconds. Calculate the mass of...
QUESTION 1 A current of 2.00A was passed through sulfuric acid for 30 mins. How many coulombs were passed through the solution? (electric charge C amperes x second) (3 significant figures, do not use scientific notation)
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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?
Question 18 (5 points) A voltaic cell is set up with silver-silver ion as one electrode and iron(II)-iron(III) ion as the other. The standard cell potential is V. Please enter your answer in decimal form, such as 0.38, and keep the correct number of significant figures.
Part B and D
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Learning Goal: To relate current, time, charge, and mass for electroplating calculations. Electroplating is a form of electrolysis in which a metal is deposited on the surface of another metal. To quantify electrolysis, use the following relationships. Electric current is measured in amperes (A), which expresses the amount of charge, in coulombs (C), that flows per second (s): 1 A 1 C/s Another unit of charge is the faraday (F),...
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?