I NEED HELP IN CHEMISTRY PLS

Question

The overall reaction in a commercial heat pack can be represented as

4Fe(s) + 3O2(g)---> 2Fe2O3(s)

(delta)H + -1652kJ

A. How much heat is released when 4.20 moles of iron are reacted with excess ?

Heat = ____  kJ

B. How much heat is released when 1.00 mole of  is produced?

Heat =  ______kJ

C. How much heat is released when 1.60 g iron is reacted with excess ?

Heat = ____ kJ

D. How much heat is released when 10.5 g  and 1.90 g  are reacted?

Heat = _____ kJ

Answer 1

4Fe(s) + 3O₂(g)---> 2Fe₂O₃(s)

A. -1652 kJ/4 mol Fe x 4.20 mol Fe = - 1735 kJ

B. -1652 kJ/2 mol Fe2O3 x 1 mol Fe2O3 = -826 kJ

C. 1.60 g Fe x 1 mol Fe/55.85 g x -1652 kJ/4 mol = -11.8 kJ

D. 10.5 g Fe x 1 mol Fe/55.85 g = 0.188 moles Fe

1.90 g O₂ x 1 mol/32 g = 0.0594 moles O₂

O₂ is limiting as the mole ratio in balanced eq. is 3:4 for O₂:Fe

0.0594 moles O2 x -1652 kJ/3 mol O2 = -32.7 kJ