Question

Magnese v phosphate reacts with 9.6 x 10^13 grams iron VII carbonate. calculate the mass of the each product produced in the process

Answer 1

For the given chemical equation,

14 Mn3(PO4)5 + 15 Fe2(CO3)7 ---> 21 Mn2(CO3)5 + 10 Fe3(PO4)7

moles of Fe2(CO3)7 reacted = 9.6 x 10^13 g/532 g/mol

                                               = 1.80 x 10^11 mol

moles of Mn2(CO3)5 formed = 1.80 x 10^11 mol x 21/15

                                              = 2.71 x 10^11 mol

mass of Mn2(CO3)5 formed = 2.71 x 10^11 mol x 409.92 g/mol

                                              = 1.11 x 10^14 g

moles of Fe3(PO4)7 formed = 1.80 x 10^11 mol x 10/14

                                              = 1.30 x 10^11 mol

mass of Fe3(PO4)7 formed = 1.30 x 10^11 mol x 832.33 g/mol

                                             = 1.08 x 10^14 g

Formulas used,

moles = grams/molar mass

grams = moles x molar mass