24.3cm3 of 0.02M KMnO4 reacted with 20.0cm3 of an iron(ii)solution a) given the half ionic...

Question

24.3cm3 of 0.02M KMnO4 reacted with 20.0cm3 of an iron(ii)solution
a) given the half ionic equations:
MnO4^-1 (aq) + 8H ^1+(aq) + 5e gives you Mn^2+ (aq) + 4H2O (L)
Fe^2+ (aq) -2e give you Fe^3+ (aq)
write a balanced equation for the reaction that takes place
b)determine:
i) number of moles of KMnO4 used
ii) number of moles of iron(ii) used
iii) concentration of iron(ii)solution in moles per litre
please explain detailed, step by step, the way a 17 year old would understand :)

Robert · Accepted Answer

24.3cm3 of 0.02M KMnO4 reacted with 20.0cm3 of an iron(ii)solution  
a) given the half ionic equations: 
MnO4^-1 (aq) + 8H ^1+(aq) + 5e gives you Mn^2+ (aq) + 4H2O (L)  
Fe^2+ (aq) -2e give you Fe^3+ (aq) 
write a balanced equation for the reaction that takes place 
b)determine:

24.3cm3 of 0.02M KMnO4 reacted with 20.0cm3 of an iron(ii)solution a) given the half ionic equations: MnO4^-1 (aq) + 8H ^1+(aq) + 5e gives you Mn^2+ (aq) + 4H2O (L) Fe^2+ (aq) -2e give you Fe^3+ (aq)...

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