# How to balance the equation H2So4 + Fe = Fe2(So4)3 + H2?

A very important aspect to keep in mind here – you don’t actually have 4 ##”So”## on the reactants’ side and 12 ##”So”## elements on the products’ side because ##”So”## ##color(red)(“is not an element”)##.
You’re dealing with the sulfate anion, ##SO_4^(2-)##, which is comprised of 1 sulfur atom, ##”S”##, and 4 oxygen atoms, ##”O”##.
This means that you can try to balance the equation either by looking at individual elements, like the other answer attempts to do, or by taking the sulfate anion as a group.
The latter options implies that you have 2 hydrogen atoms, 1 sulfate group, and 1 iron atom on the left side of the equation, and 2 iron atoms, 2 hydrogen atoms, and 3 sulfate groups on the right side of the equation.
##H_2SO_4 + Fe -> Fe_2(SO_4)_3 + H_2##
Balance the sulfate group first and focus on the rest of the species afterwards. So, you have three times more sulfate groups on the right hand side of the equation ##->## multiply the compound that contains the sulfate group by 3 on the left hand side.
##color(red)(3)H_2SO_4 + Fe -> Fe_2(SO_4)_(color(red)(3)) + H_2##
By multiplying this compound by 3, you’ve increased the number of hydrogen atoms on the left hand side to 6 ##->## multiply the hydrogen on the right hand side by 3 to balance them out.
##color(red)(3)H_(color(blue)(2))SO_4 + Fe -> Fe_2(SO_4)_(color(red)(3)) + color(red)(3)H_color(blue)(2)##
Finally, you’ve got 2 iron atoms on the right hand side ##->## multiply the iron by 2 on the left hand side to balance them out
##color(red)(3)H_(color(blue)(2))SO_4 + color(green)(2)Fe -> Fe_(color(green)(2))(SO_4)_(color(red)(3)) + color(red)(3)H_color(blue)(2)##

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