The problem says, for each of the following unbalanced equations, calculate how many milligrams of each product would be produced by complete reaction of 10.0 mg of the reactant indicated in the boldfance. Indicate clearly the mole ratio used for the conversion.
the FeSo4 of the reactant side is boldfaced.
FeSO4(aq)+ K2CO3(aq)----->FeCO3(S)+K2SO4(aq)
can someone explain in depth what to do? all i know is that i am suppose to balance the equation first, but the equation already seems to be balanced.
the FeSo4 of the reactant side is boldfaced.
FeSO4(aq)+ K2CO3(aq)----->FeCO3(S)+K2SO4(aq)
can someone explain in depth what to do? all i know is that i am suppose to balance the equation first, but the equation already seems to be balanced.