Bismuth can be electrolytically reduced according to the following reaction:
BiO(+)+ 2H(+)+ 3e¯ >>> Bi + H2O
How many grams of bismuth can be reduced by applying a 5.60 A current for 23.8 min. to a solution containing BiO+
ions
(assuming 100% efficiency)?
96,485 Coulombs can plate out approx 209/3 grams Bi. You need a better answer than that estimate.
How many coulombs do you have? That's
C = amperes x seconds = approx 5.60 x 23.8 x 60 s/min = ?
209/3 x ?coulombs/96,485 = g plated out.
To determine the number of grams of bismuth that can be reduced, you'll need to use the formula:
q = It
where:
q represents the total charge in coulombs (C),
I is the current in amperes (A), and
t is the time in seconds (s).
First, convert the time from minutes to seconds.
23.8 min * 60 s/min = 1428 s
Next, calculate the total charge (q) using the formula:
q = It
q = 5.60 A * 1428 s
q = 7996.8 C
Since 3 moles of electrons are needed to reduce 1 mole of BiO+ ions, and 1 mole of bismuth (Bi) has a mass of approximately 208.98 g (according to the atomic mass of bismuth), we can determine the number of grams of bismuth using the following steps:
1. Calculate the number of moles of electrons:
moles of electrons = q / Faraday's constant
The Faraday's constant (F) is approximately 96,485 C/mol, so:
moles of electrons = 7996.8 C / 96485 C/mol
moles of electrons ≈ 0.0828 mol
2. Calculate the number of moles of bismuth (Bi):
moles of bismuth (Bi) = moles of electrons / 3
moles of bismuth (Bi) ≈ 0.0828 mol / 3
moles of bismuth (Bi) ≈ 0.0276 mol
3. Calculate the mass of bismuth (Bi) using the molar mass:
mass of bismuth (Bi) = moles of bismuth (Bi) * molar mass of bismuth (Bi)
mass of bismuth (Bi) ≈ 0.0276 mol * 208.98 g/mol
mass of bismuth (Bi) ≈ 5.76 g
Therefore, approximately 5.76 grams of bismuth can be reduced by applying a 5.60 A current for 23.8 min to a solution containing BiO+ ions, assuming 100% efficiency.