Silver can be plated out of a solution containing Ag+ according to the half-reaction
Ag+(aq)+e−→Ag(s)
How much time (in minutes) does it take to plate 19 g of silver using a current of 4.8 A ?
Express the time to two significant figures and include the appropriate units.
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Silver can be plated out of a solution containing Ag+ according to the half-reaction Ag+(aq)+e−→Ag(s) How...
Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction. Cu2+(aq)+2e−→Cu(s) How much time would it take for 329 mg of copper to be plated at a current of 7.1 A ? Express your answer using two significant figures.
Part A and B Please show all of the steps Analysis of Electroplating 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...
Nickel can be plated from aqueous solution according to the following half reaction. How long would it take in seconds) to plate 3.2 g of nickel at 50.0 Amps ? A.W.NI - 58.7 g/mol Ni 2+(aq) + 2 e-- NI(S) a. 2100 seconds b. 21.0 seconds C 1.1 x 104 seconds d. 210 seconds e. 105 seconds
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...
The addition of hydroiodic acid to a silver nitrate solution precipitates silver iodide according to the reaction: AgNO3(aq)+HI(aq)→AgI(s)+HNO3(aq) When 50.0 mL of 5.00×10−2M AgNO3 is combined with 50.0 mL of 5.00×10−2M HI in a coffee-cup calorimeter, the temperature changes from 22.40 ∘C to 22.91∘C. Part A Calculate ΔHrxn for the reaction as written. Use 1.00 g/mL as the density of the solution and Cs=4.18J/(g⋅∘C) as the specific heat capacity of the solution. Express the energy to two significant figures and include...
Chapter 19 Homework tem 19 Review I Constants Silver can be electroplated at the cathode of an electrolysis cel by the half-reaction. Ag (aq) + e + Ag(s) You may want to reference (Pages 920-925) Section 19.8 while completing this problem. Silver can be electroplated at the cathode of an electrolysis cell according to the following half-reaction: Ag+ (aq) + e + Ag(s) What made of silver plates onto the cathode when a current of 8.2 A flows through the...
Question 12 0.5 pts Silver can be electroplated at the cathode of an electrolys is cell by the half- reaction. Ag*(aq) eAg(s) What mass of silver would plate onto the cathode if a current of 6.8A flowed through the cell for 72 min? Mass Ag(s) 4.11 grams Mass Ag(s) 6.81 grams Mass Ag(s) 16.42 grams Mass Ag(s) 32.84 grams Mass Ag(s) 65.68 grams Mass Ag(s) 72.00 grams
help with part B please precipitates out of solution according to the When solutions of silver nitrate and calcium chloride are mixed, silver chloride equation ble 2AgNO,(ag) + CaCl(aq) 2AgCls) + Ca(NO,)(ag) ways ity, M ▼ Part B The reaction described in Part A required 3.21 L of calcium chloride. What is the concentration of this calcium chioride solution? Express your answer with the appropriate units. View Available Hint(s) 1444 Submit Incorrect; Try Again; 3 attempts remaining
If the following half-reactions are used in an electrolytic cell: Ag+(aq) + e− ⟶ Ag(s) Eo = 0.80 V Ca2+(aq) + 2 e− ⟶ Ca(s) Eo = −2.76 V Click here for a copy of Final Exam cover sheet. 1) The metal solid that is plated out at the cathode is [Ag(s), Ca(s)] 2) It would take [3, 8. 16] hours to deposit 60 g of the solid with a current of 5.0 A.
Copper can be electroplated at the cathode of an electrolysis cell by the half-reaction: Cu2+(aq)+2e−→Cu(s) How much time would it take for 348 mgmg of copper to be plated at a current of 6.3 AA?