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3. How many minutes are required to electroplate 25.0 g of metallic Cu from aq. CuSO4...
1a. How much current is required to electroplate a metal surface with 0.123 g nickel metal...
1a. How much current is required to electroplate a metal surface with 0.123 g nickel metal from a solution of Ni2+(aq) in 101 seconds? = _ A 1b. Molten CaCl2 can be electrolyzed to form metallic Ca. For what duration should an electrolysis be performed at a current of 2.27 A in order to produce 15.6 g Ca? = _ s
how many Cu2+ ions are in a mole of CuSO4 Part A 21 How many Cu...
how many Cu2+ ions are in a mole of CuSO4
Part A 21 How many Cu ions are in a mole of CuSO4? Express your answer using four significant figures. N= Submit My Answers Give Up
Copper(II) ions can be displaced by aluminum metal. 3 CuSO4(aq) + 2 Al(s) → Al2(SO4)3(aq) +...
Copper(II) ions can be displaced by aluminum metal. 3 CuSO4(aq) + 2 Al(s) → Al2(SO4)3(aq) + 3 Cu(s) How many grams of Al would be needed to displace all of the copper ions in 40.5 mL of 0.420 M CuSO4? How many grams of Cu would be recovered from the copper ions in 40.5 mL of 0.420 M CuSO4?
• 18.55 A steady current was passed through molten CoSO4 until 2.35 g of metallic cobalt...
• 18.55 A steady current was passed through molten CoSO4 until 2.35 g of metallic cobalt was pro- duced. Calculate the number of coulombs of elec- tricity used. • 18.59 The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a CuSO4 solution. From this information, calculate the molar mass of copper. 18.87 In a certain electrolysis experiment involving Al+ ions, 60.2 g of Al is recovered when a current of 0.352 A...
14. Metallic iron can be made by the electrolysis of molten Fe2O3. How many minutes are...
14.
Metallic iron can be made by the electrolysis of molten
Fe2O3.
How many minutes are needed to plate out 20.00 g of Fe from molten
Fe2O3 using 5.55 A current? Use F = 96,500
C/mol for Faraday's constant. The unbalanced chemical reaction
representing this electrolysis is shown below:
Fe2O3
Fe + O2
pls explain
a) This process takes 1.09e+02 minutes.
b) This process takes 1.87e+04 minutes.
c) This process takes 3.11e+02 minutes.
d) This process takes 3.63e+01 minutes.
e)...
Introduction The chemical reactions involved in this experiment are: CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s)...
Introduction The chemical reactions involved in this experiment are: CuSO4(aq) + Zn(s) → ZnSO4(aq) + Cu(s) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) The copper on the surface quickly reacts with oxygen according to the following reaction: 2Cu(s) + O2(g) → 2CuO(s) Experimental Procedure Dissolve completely about 0.5 to 0.7 g of copper (II) sulphate pentahydrate in about 10 to 20 mL of deionized water. Calculate the amount of zinc powder that must be added to a copper sulfate solution...
Please use railroad tracks for work, thank you. 1. How many faradays are transferred in an...
Please use railroad tracks for work, thank you.
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...
In order to produce 31.8 g of Cu by the reaction H2e) CuO Cu H20, how many liters of hydrogen would be required if the...
In order to produce 31.8 g of Cu by the reaction H2e) CuO Cu H20, how many liters of hydrogen would be required if the reaction were run at 760. torr and 20.0°C? what is the density of CO2 gas at STP? at 20.0 C and 1.0 atm pressure?
5. How long would it take to electroplate a flute with 28.3 g of silver (107.87...
5. How long would it take to electroplate a flute with 28.3 g of silver (107.87 g/mol) at a constant current of 2.0 amps using AgNO3?
The following reactions should be useful: i. Cu(s) + 4HNO3(aq) + Cu(NO.) + 2NO2(g) + H,00...
The following reactions should be useful: i. Cu(s) + 4HNO3(aq) + Cu(NO.) + 2NO2(g) + H,00 ii 2HNO, (aq) + Na.co,(s) → H2O(l) + CO2(g) + 2NaNO3(aq) ii. Cu(NO)2(aq) + Na.co, (s) → Cuco,(s) + 2NaNO3(aq) iv. Cuco,(s) + 2HCl(aq) → CuCl(aq) + H2O(1) + CO2(g) v. CuCl(aq) +Cu(s) → 2CuCl(s) 2. How many grams of copper will be produced if 25.0 mL of a 0.156 M CuSO, solution reacts with 7.89 g of zinc according to the given equation....
how many Cu2+ ions are in a mole of CuSO4
Part A 21 How many Cu ions are in a mole of CuSO4? Express your answer using four significant figures. N= Submit My Answers Give Up
• 18.55 A steady current was passed through molten CoSO4 until 2.35 g of metallic cobalt was pro- duced. Calculate the number of coulombs of elec- tricity used. • 18.59 The passage of a current of 0.750 A for 25.0 min deposited 0.369 g of copper from a CuSO4 solution. From this information, calculate the molar mass of copper. 18.87 In a certain electrolysis experiment involving Al+ ions, 60.2 g of Al is recovered when a current of 0.352 A...
14.
Metallic iron can be made by the electrolysis of molten
Fe2O3.
How many minutes are needed to plate out 20.00 g of Fe from molten
Fe2O3 using 5.55 A current? Use F = 96,500
C/mol for Faraday's constant. The unbalanced chemical reaction
representing this electrolysis is shown below:
Fe2O3
Fe + O2
pls explain
a) This process takes 1.09e+02 minutes.
b) This process takes 1.87e+04 minutes.
c) This process takes 3.11e+02 minutes.
d) This process takes 3.63e+01 minutes.
e)...
Please use railroad tracks for work, thank you.
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...
5. How long would it take to electroplate a flute with 28.3 g of silver (107.87 g/mol) at a constant current of 2.0 amps using AgNO3?
The following reactions should be useful: i. Cu(s) + 4HNO3(aq) + Cu(NO.) + 2NO2(g) + H,00 ii 2HNO, (aq) + Na.co,(s) → H2O(l) + CO2(g) + 2NaNO3(aq) ii. Cu(NO)2(aq) + Na.co, (s) → Cuco,(s) + 2NaNO3(aq) iv. Cuco,(s) + 2HCl(aq) → CuCl(aq) + H2O(1) + CO2(g) v. CuCl(aq) +Cu(s) → 2CuCl(s) 2. How many grams of copper will be produced if 25.0 mL of a 0.156 M CuSO, solution reacts with 7.89 g of zinc according to the given equation....
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