How many moles of Fe2+ can be oxidized by 0.043 moles MnO4-?

the redox reaction that i balanced was:


2Mno4- + 5HC2O4- + 11H+ --%26gt; 2Mn2+ + 8H2O + 10CO2


i got as far as converting the moles of MnO4- to grams; is that even nescesary? or would i just use the the ration to find the moles of Fe2+? could someone please help? thanks!

How many moles of Fe2+ can be oxidized by 0.043 moles MnO4-?
The equation is not this ( where is Fe2+? )





but it is :





8H+ + MnO4- + 5Fe2+ %26gt;%26gt; Mn2+ + 5Fe3+ +4H2O





the ratio between MnO4- and Fe2+ is 1 : 5





1 : 5 = 0.043 : x





x = 0.215 moles Fe2+ that can be oxidized
Reply:You don't need grams, just the ratio. MnO4- has room for 5 electrons. Depending on what's happening to your iron, and I suspect it's going from 2+ to 3+ (You gave the wrong equation); if so, you can oxidixe 5 times your .043 moles as each mole of permanganate can oxidize on Fe2+ to Fe3+.

street fighting