determine the number of electrons required to deposit 6.4g of copper from an aqueous solution of copper II sulphate
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It will take 1 mole of electrons (6.02 x 10^23 electrons) to deposit 1 equivalent weight of Cu.
One equivalent weight of Cu is 64/2 = 32 grams. You have 6.4/32 = 0.2 equivalent.
To determine the number of electrons required to deposit 6.4g of copper from an aqueous solution of copper II sulfate, we need to use the concept of electrochemical equivalence.
1. Start by calculating the molar mass of copper (Cu):
- The molar mass of copper (Cu) is 63.55 g/mol.
2. Convert the mass of copper (Cu) into moles:
- Moles = Mass / Molar mass of copper (Cu)
- Moles = 6.4g / 63.55 g/mol ≈ 0.101 mol
3. Use the balanced chemical equation for the deposition of copper (Cu) from copper II sulfate (CuSO4):
- Cu2+ + 2e- → Cu
4. From the balanced chemical equation, we can see that for every 2 moles of electrons (2e-), 1 mole of copper (Cu) is deposited.
5. Calculate the number of moles of electrons required to deposit the given amount of copper (Cu):
- Moles of electrons = Moles of copper / 2
- Moles of electrons = 0.101 mol / 2 ≈ 0.051 mol
6. Finally, calculate the number of electrons using Avogadro's number:
- Number of electrons = Moles of electrons × Avogadro's number
- Number of electrons = 0.051 mol × 6.022 × 10^23 electrons/mol
- Number of electrons ≈ 3.08 × 10^23 electrons
Therefore, approximately 3.08 × 10^23 electrons are required to deposit 6.4g of copper from an aqueous solution of copper II sulfate.
To determine the number of electrons required to deposit 6.4g of copper from an aqueous solution of copper II sulfate (CuSO4), we need to understand the concept of Faraday's law of electrolysis.
Faraday's law states that the amount of chemical reaction occurring at an electrode is directly proportional to the amount of electric charge that passes through the electrode. The electric charge is measured in coulombs (C), and the relationship between electric charge (Q), current (I), and time (t) is given by the equation Q = I * t.
To calculate the number of electrons (n) involved in the electrochemical reaction, we need to convert the amount of substance (6.4g of copper) to moles using its molar mass. The molar mass of copper (Cu) is 63.55 g/mol.
1. Calculate the moles of copper (Cu):
Moles = Mass / Molar mass
Moles = 6.4g / 63.55 g/mol
Moles ≈ 0.101 mol
2. Determine the number of electrons involved in the reaction:
From the chemical equation of the reaction, we know that copper (Cu2+) gains two electrons (2e-) to form elemental copper (Cu).
Therefore, the number of electrons (n) required = 2 * Moles of copper
n = 2 * 0.101 mol
n ≈ 0.202 mol
3. Convert the number of moles to the number of electrons:
1 mol of electrons contains Avogadro's number of electrons, which is approximately 6.022 x 10^23 electrons/mol.
Number of electrons = n * Avogadro's number
Number of electrons ≈ 0.202 mol * 6.022 x 10^23 electrons/mol
Number of electrons ≈ 1.215 x 10^23 electrons.
Therefore, approximately 1.215 x 10^23 electrons are required to deposit 6.4g of copper from an aqueous solution of copper II sulphate.