What is the balanced equation when aluminum reacts with copper (ii) sulfate? i don't know how to do this
1 answer:
Here Cu (II) reduced to Cu (0). Al would be strong reducing agent to do so. Now ... Compare Al and Cu reduction potentials. Al3+(aq) + 3 e– ----> Al(s) -1.66
Cu(OH)2(s) + 2 e– ----> Cu(s) + 2 OH–(aq) -0.36. It implies that reduction potential of Cu is more than Al hence this reaction is not feasible bcuz copper is a reducing agent ( oxidize itself or reduces others). But still you can balance...practically this reaction seems impossible bcuz of above reason.
Cu(OH)2(s) + 2 e– ----> Cu(s) + 2 OH–(aq) -0.36. It implies that reduction potential of Cu is more than Al hence this reaction is not feasible bcuz copper is a reducing agent ( oxidize itself or reduces others). But still you can balance...practically this reaction seems impossible bcuz of above reason.
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Answer :
(a) The moles of water produced are 145.35 moles.
(b) The mass of oxygen needed are 3080.8 grams.
<u>Solution for part (a) : Given,</u>
Moles of = 16.15 moles
First we have to calculate the moles of
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 2 moles of react to give 18 moles of
So, 16.15 moles of react to give
moles of
The moles of water produced are 145.35 moles.
<u>Solution for part (b) : Given,</u>
Mass of = 878 g
Molar mass of = 114 g/mole
Molar mass of = 32 g/mole
First we have to calculate the moles of .
Now we have to calculate the moles of
The balanced chemical reaction is,
From the balanced reaction we conclude that
As, 2 moles of react with 25 moles of
So, 7.702 moles of react with
moles of
Now we have to calculate the mass of .
The mass of oxygen needed are 3080.8 grams.