Chemistry

One reaction of iron with hydrochloric acid is represented by the following
thermochemical equation.
Fe(s) + 2HCl(aq) ? FeCl2(aq) + H2(g); (Delta)H°= –87.9 kJ
How much heat is liberated at constant pressure if 0.215 g of iron reacts with 40.4 mL of
0.579 M HCl?
How much heat is liberated at constant pressure when 28 g of calcium oxide reacts with 86.5 L of carbon dioxide gas measured at 1 atm pressure and 25C( R=0.0821 L.atm\(K.mol) CaO(s)+CO2(g)---CaCO3(s);delta H=-178.3 kJ
These are final two HW problems I can not get the correct answer on either. Been waking on them for two days. Help show all steps so I can find my mistakes.

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asked by Raul
  1. The better idea is for you to type and let us check. It's much faster that way. However, I'll split it with you and do the first.
    mols Fe = grams/molar mass. (You need to check that Fe is the limiting reagent.(It is.)
    Basically you read it this way. If 87.9 kJ heat is liberated for 1 mol (55.85) g Fe, how much is liberated for 0.215.
    That's 87.9 kJ x (0.215/55.85) = ?kJ.

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