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:
-1
Explanation:
The relation between Kp and Kc is given below:
Where,
Kp is the pressure equilibrium constant
Kc is the molar equilibrium constant
R is gas constant , 0.082057 L atm.mol⁻¹K⁻¹
T is the temperature in Kelvins
Δn = (No. of moles of gaseous products)-(No. of moles of gaseous reactants)
For the first equilibrium reaction:
<u>Δn = (No. of moles of gaseous products)-(No. of moles of gaseous reactants) = (2+1)-(2+2) = -1 </u>
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Answer:
Isotopes of an element are atoms of the same element that have different number of neutrons.
