- Scan Question
- + Post
- Get Coins
A spoon was silver-plated electrolytically in a AgNO3 solution. If 0.750 g of Ag was deposited on the spoon at a constant current of 20.0 mA, how long (in hours) did the electrolysis take? (1 mA = 1x10–3 A)
Ag+(aq) + e -------> Ag(s)
1mole of electrons is required to deposite 1mole of Ag+
Number of moles of Ag+ = 0.750g /107.87g/mol = 0.006953mol
number of moles of electrons required = 0.006953mol
Number of Columbs required = 0.006953mol × 96485C/mol = 670.86C
20.0mA = 0.0200A
1Ambs = 1Coloumb per second
0.0200A = 0.0200Couloumbs per second
Time required for electrolysis = 670.86C/0.0200C/s = 33543s = 9.32 hr
A spoon was silver-plated electrolytically in a AgNO3 solution. If 0.750 g of Ag was deposited...
Question 11 An antique spoon is to be silver-plated. How long will it take to plate 21.4 g of Ag (atomic mass=107.9 g/mol) from a solution of AgNO3 using a current of 10.0 amp? a. 63.8 min b. 31.9 min O c. 161 min Od 1.15 x 105 min O e. 80.4 min Moving to another question will save this response. Question 12 A 25.0 ml sample of 0.20 M Formic Acid (HCO2H, aq) is titrated with 0.10 M KOH(aq)....
What mass (g) of silver will be obtained when an aqueous silver nitrate (AgNO3) solution is electrolyzed for 30.0 minutes with a constant current of 5.40 A? 10.9 g Ag formed ♡ 12.3 g Ag formed 3.22 g Ag formed 5.72 g Ag formed