The first part of the problem asks this: Calculate the heat (?H rxn ) in kJ of t

Question

The first part of the problem asks this:

Calculate the heat (?Hrxn ) in kJ of the following reaction:

2Fe2O3(s)   +   2CO(g)  -->  4FeO(s)  +  2CO2(g)

I think that I have calculated this correctly. This is what I have done so far.

2(-824.2)+2(-110.5)= -1869.4        and        4(-271.9)+2(-393.5)= -1874.6

Delta H reaction = -1874.6-(-1869.4)= -5.2 kJ

Then the next question asks:

If you start with 20.00 g of Fe2O3 in the reaction in Question 1 above and react it in excess CO, how much heat (in kJ) is gained or released?  (Use the proper sign to show if heat is gained or released.)

I am not sure how to go about solving for this and I keep getting the answer wrong so I would really appreciate any help!

The first part of the problem asks this: Calculate the heat (?Hrxn ) in kJ of the following reaction: 2Fe2O3(s) + 2CO(g) --> 4FeO(s) + 2CO2(g) I think that I have calculated this correctly. This is what I have done so far. 2(-824.2)+2(-110.5)= -1869.4 and 4(-271.9)+2(-393.5)= -1874.6 Delta H reaction = -1874.6-(-1869.4)= -5.2 kJ Then the next question asks: If you start with 20.00 g of Fe2O3 in the reaction in Question 1 above and react it in excess CO, how much heat (in kJ) is gained or released? (Use the proper sign to show if heat is gained or released.) I am not sure how to go about solving for this and I keep getting the answer wrong so I would really appreciate any help!

Explanation / Answer

I am assuming that your calculation in finding dH is correct

now 20 g Fe2O3 is reacted

molarmss of Fe2O3 = 159.7

Now mole of Fe2O3 = 20/159.7 = 0.12523

for one mole -5.2 kJ of energy is released (released because the sign is negative)

hence energy released = 0.12523*-5.2 = -0.65122 KJ

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