How many grams of copper metal can be obtained by passing a current of 1.50 amp through a solution of Cu^2+ (aq) for 45 minutes?
Please show calculation steps!
Please show calculation steps!
-
6.242 × 10^18 electrons passing a given point each second constitutes one ampere
Copper in a solution is Cu+2 ions, which need 2 electrons to be reduced to Cu atoms.
1.5 amps == 1.5 * 6.242 × 10^18 electrons passing a given point each second
45 minutes = 45 * 60 = 2700 seconds
1.5 amps * 2700 seconds * 6.242 × 10^18 electrons /amp*second = 2.53*10^22 electrons
2.53 * 10^22 electrons / 2 electrons/Cu atom = 1.265* 10^22 Cu atoms
6.02 * 10^ 23 atoms = 1mole
1.265* 10^22 Cu atoms / 6.02 * 10^ 23 atoms/mole = 0.021 moles of Cu
0.021 moles * 63.456 grams/mole = 1.33 grams of Cu
Why did the person below copy my answer??
Copper in a solution is Cu+2 ions, which need 2 electrons to be reduced to Cu atoms.
1.5 amps == 1.5 * 6.242 × 10^18 electrons passing a given point each second
45 minutes = 45 * 60 = 2700 seconds
1.5 amps * 2700 seconds * 6.242 × 10^18 electrons /amp*second = 2.53*10^22 electrons
2.53 * 10^22 electrons / 2 electrons/Cu atom = 1.265* 10^22 Cu atoms
6.02 * 10^ 23 atoms = 1mole
1.265* 10^22 Cu atoms / 6.02 * 10^ 23 atoms/mole = 0.021 moles of Cu
0.021 moles * 63.456 grams/mole = 1.33 grams of Cu
Why did the person below copy my answer??
-
6.242 × 10^18 electrons passing a given point each second constitutes one ampere
Copper in a solution is Cu+2 ions, which need 2 electrons to be reduced to Cu atoms.
1.5 amps == 1.5 * 6.242 × 10^18 electrons passing a given point each second
45 minutes = 45 * 60 = 2700 seconds
1.5 amps * 2700 seconds * 6.242 × 10^18 electrons /amp*second = 2.53*10^22 electrons
2.53 * 10^22 electrons / 2 electrons/Cu atom = 1.265* 10^22 Cu atoms
6.02 * 10^ 23 atoms = 1mole
1.265* 10^22 Cu atoms / 6.02 * 10^ 23 atoms/mole = 0.021 moles of Cu
0.021 moles * 63.456 grams/mole = 1.33 grams of Cu
Copper in a solution is Cu+2 ions, which need 2 electrons to be reduced to Cu atoms.
1.5 amps == 1.5 * 6.242 × 10^18 electrons passing a given point each second
45 minutes = 45 * 60 = 2700 seconds
1.5 amps * 2700 seconds * 6.242 × 10^18 electrons /amp*second = 2.53*10^22 electrons
2.53 * 10^22 electrons / 2 electrons/Cu atom = 1.265* 10^22 Cu atoms
6.02 * 10^ 23 atoms = 1mole
1.265* 10^22 Cu atoms / 6.02 * 10^ 23 atoms/mole = 0.021 moles of Cu
0.021 moles * 63.456 grams/mole = 1.33 grams of Cu
-
I won't give you the answer, but I'll give you guidance towards how to solve it.
If you divide the current by the time (in seconds) you've got an answer in coulombs. Using Faraday's constant (96500 C/mol) you get moles of electrons involved in this process. Since you are using Cu^2+ you have 2 moles of electrons per mole of copper. From here, you can do a simple molar mass conversion to get the mass of deposited copper.
Hope this helped.
If you divide the current by the time (in seconds) you've got an answer in coulombs. Using Faraday's constant (96500 C/mol) you get moles of electrons involved in this process. Since you are using Cu^2+ you have 2 moles of electrons per mole of copper. From here, you can do a simple molar mass conversion to get the mass of deposited copper.
Hope this helped.