How Much Energy Results from Reacting 2.0kg of Hydrogen with 38kg of Fluorine?

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The reaction of 2.0 kg of hydrogen with 38 kg of fluorine produces approximately 500 kJ/mol of energy. To calculate the total energy released, one must first determine the number of moles of each reactant, considering that both hydrogen and fluorine are diatomic. The resulting energy from this reaction is calculated to be 5.0 x 10^5 kJ. Understanding the stoichiometry of the reaction is crucial for accurate energy calculations. This discussion emphasizes the importance of mole calculations in determining energy output in chemical reactions.
Koyuki
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the reaction of H and F produces about 500 kj/mol of energy:

how much energy is produced by the reaction of 2.0kg of H with 38 kg of F to produce 2 kmol of HF?

The answer is 5.0x 10 to the exponent 5 kJ... but I'm not sure why...

Please help! Thanks!
 
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This is chemistry and should be in the chemistry forums, but try calculating the number of moles of each reactant. Remember Hydrogen and Florine are diatomic.
 
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