Chem 1 thermochemistry problem? Am I doing this right?

AI Thread Summary
To calculate the heat released when 5.00 g of aluminum reacts with chlorine, first convert grams of aluminum to moles using its molar mass. Then, apply the enthalpy change (delta H) of -1408.4 kJ for the reaction of 2 moles of Al. Since the reaction involves 2 moles of Al, divide the delta H by 2 to find the heat released per mole. Finally, multiply the heat per mole by the number of moles of aluminum from your conversion. This approach accurately determines the heat released in the reaction.
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Homework Statement



When aluminum reacts with chlorine
how much heat in KJ is released on reaction of 5.00 g of Al
for the following reaction:
2AL (s) + 3 CL2(g) ----->2AlCl3 (s)
delta h = -1408.4



Homework Equations





The Attempt at a Solution



Is it right if you start multiplying the delta H by the number of grams of Al , and by doing that by first converting grams of Al to moles? It's hard to tell you if you would divide by 2 at all? 2Al has something to do with it maybe?
 
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Think about it this way - you are given amount of heat evolving per 2 moles of Al reacting.
 

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