5.06 moles of iron(II)phosphate, Fe₃(PO₄)₂, are produced in a reaction. What mass of iron(II)phosphate is produced?

Question

Quizplus · Accepted Answer

We need to use the mole-to-mass conversion formula which is:
mass = mole x molar mass

The molar mass of Fe3(PO4)2 can be calculated by adding the molar mass of each element in the compound:
molar mass of Fe = 55.85 g/mol
molar mass of P = 30.97 g/mol
molar mass of O = 15.99 g/mol
Total molar mass = (2 x molar mass of Fe) + (3 x molar mass of P) + (8 x molar mass of O)
= (2 x 55.85 g/mol) + (3 x 30.97 g/mol) + (8 x 15.99 g/mol) = 399.88 g/mol

Now, we can use the mole-to-mass conversion formula to calculate the mass of Fe3(PO4)2 produced:
mass = mole x molar mass
mass = 5.06 mol x 399.88 g/mol
mass = 2,020.728 g or 2.02 kg

However, the answer choices are in grams, so we need to convert the answer to grams and round to the nearest tenth:
mass = 2.02 kg x 1000 g/kg = 2,020 g
mass = 1.81 × 10^3 g (rounded to the nearest tenth)

Therefore, the best choice is C, 1.81 × 10^3 g, because it is the only answer that matches the calculation using the mole-to-mass conversion formula.

506 Moles of Iron(II)phosphate, Fe3(PO4)2, Are Produced in a Reaction

506 Moles of Iron(II)phosphate, Fe₃(PO₄)₂, Are Produced in a Reaction