What is the average current passing through a solution of NiSO4 if 3.49 g of Ni were deposited in 8.71 hours?
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What is the average current passing through a solution of NiSO4 if 3.49 g of Ni...
25.0 mL of 0.100 M NiSO4 solution is added to 50.0-mL of a 0.080 M NaOH solution. NiSO4(aq) + 2 NaOH(aq) -> Ni(OH)2(s) + Na2SO4(aq) a. What is the limiting reagent? b. What is the mass of precipitate formed? c. After the reaction is complete, calculate the concentration of the reactant remaining in solution. ( NiSO4 = 158.8 g/mol | NaOH = 40.0 g/mol | Ni(OH)2 = 92.7 g/mol )
A current of 5.65 A is passed through a Ni(NO3)2 solution. How long (in hours) would this current have to be applied to plate out 5.40 g of nickel?
A current of 5.26 A is passed through a Ni ( NO 3 ) 2 solution for 1.90 h . How much nickel is plated out of the solution? mass of nickel: g
If the average current passing through the secondary coil of the transformer with 40 turns and a secondary voltage of 24-V AC is 10 A, what average current is passing through the primary coil that makes 200 turns and has a primary voltage of 120-V AC?
An inexpensive and accurate method of measuring the quantity of electricity passing through a circuit is to pass it through a solution of a metal ion and weigh the metal deposited. A silver electrode immersed in an Ag+ solution weighs 1.7854 g before the current passes and weighs 1.9283 g after the current has passed. How many coulombs have passed?
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5. How many grams of nickel would be electroplated by passing a constant current of 7.2 A through a solution of NiSO4 for 90.0 min? (4pts) Ans:
How many kg of Ni can be produced from a solution of Ni2+ by a current of 1200 amps over a period of 36 hours? F = 96,485 amp-sec / mole e- Ni = 58.69 g/mol What is n for this reaction? _________ How many moles of electrons were transferred? _____________ How many moles of Ni were produced? _______________ How many kg of Ni were produced? ________________ Is this an oxidation or a reduction process? ________________
2.60 g of a metal (M) were collected after passing a current of 5.00 A for a duration of 30 min through a solution of an M2 salt. What is the identity of the metal? Fe a. b. Cu Zn C. d. Mg
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1. How many faradays are transferred in an electrolytic cell when a current of 2.0 A flows for 12 hours? (1 faraday = 96,500 C) 2. A metal object is to be gold-plated by an electrolytic procedure using aqueous AuCl3 electrolyte. How much gold may be deposited in 3.0 min by a constant current of 10.0 A? 3. What mass of nickel may be electroplated by passing a constant current of 7.2...
3. Calculate the current needed to deposit 2. 45 grams of Ni in 3 hours and 15 minutes from a Ni(NO3)2 solution. 4. Using the calculated current from question 3, What mass of Nickel would be deposited with that same current over 8 hours, if the deposition was 68% efficient? 5. In an electrolytic cell, if the anode is an active electrode, would its mass increase or decrease as the reaction progresses?