In: Chemistry
If delta rG for the following reaction is -1880 kJ, calculate Ecell. How many electrons are transferred in this equation?
2MnO4- (aq) + 5Fe (s) + 16H+ (aq) ----> 2 Mn2+ (aq) + 5 Fe2+ (aq) +8H20 (l)
(I am trying to find n electrons in order to plug into the equation: Ecell=DeltaG/nF)
Oxidation number of each element in MnO4-1 is
O=-2
Mn=+7
Oxidation number of each element in Fe is
Fe=0
Oxidation number of each element in Mn+2 is
Mn=+2
Oxidation number of each element in Fe+2 is
Fe=+2
Oxidation number of each element in reactant is
O=-2
Mn=+7
Fe=0
Oxidation number of each element in product is
Mn=+2
Fe=+2
Mn in MnO4- has oxidation state of +7
Mn in Mn+2 has oxidation state of +2
So, Mn in MnO4- is reduced to Mn+2
Number of electron transferred per Mn = 5
there are 2 Mn.
So, number of electron = 10
Fe in Fe has oxidation state of 0
Fe in Fe+2 has oxidation state of +2
So, Fe in Fe is oxidised to Fe+2
Number of electron transferred per Fe = 2
there are 5 Fe.
So, number of electron = 10
Either way we can find out the number of electrons
It is 10