When 10.00g of iron is burned in O2 to form Fe3O4, enough heat is generated to raise the temperature of 784g of water from 18.0degC to 38.0degC. Calculate the heat of formation of Fe3O4 under these conditions
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brittany
ANSWERS: 2
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This looks like a homework problem. So, I am not going to do it for you. I will, however, tell you how to do it. First of all, they don't seem to tell you what units of energy to use. So, I will suggest that you use calories. This is the easiest unit of energy to work with when you are working with water because it take 1 calorie to change the temperature of 1 gram of water by 1° celsius. So, it is all ones and ones are easy to work with when you are multiplying and dividing. So, keeping this in mind, what you need to do is find the total amount of heat absorbed by the water. To get this, you simply have to multiply the temperature change by the total mass of water. This will give you the amount of energy released by burning 10 grams of iron. the answer that you want will have to be expressed in terms of the amount of energy is released per gram of iron. So how do you get from the total per 10 grams to the total per gram? If you will now do the rest of the work to get the answer and post as a comment to this question, then I will tell you if you got it right or not.
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Well, i know that i am supposed to use the original equation q=m x c x delta T which would give: 784 x 4.18 x 20degrees celcius this gives 65542.4 J. I believe that the answer needed to be in kJ. After this point i am stuck.
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