Calculate Energy Req'd for 2 kmol HF from 2.0kg H and 38 kg F

[anias]

I Have A Question about FUSION! Please Help!

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?

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


PLEASE HELP!
thanks for your time =D

 

[Mk]

Please do not double post, its agaist the rules. If you accidentally do it, you can delete the post of which you select.

 

[sir-pinski]

Hello!

To calculate the energy required for 2 kmol of HF from 2.0kg H and 38 kg F, we first need to determine the moles of H and F present.

1 kmol = 1000 moles, so 2 kmol = 2000 moles.

To find the moles of H, we use the molar mass of H, which is 1 g/mol.

2.0 kg H = 2000 g H
2000 g H / 1 g/mol = 2000 moles H

To find the moles of F, we use the molar mass of F, which is 19 g/mol.

38 kg F = 38,000 g F
38,000 g F / 19 g/mol = 2000 moles F

Now, we can use the balanced chemical equation for the reaction of H and F to determine the energy produced.

2H2 + 2F2 → 4HF

From the equation, we can see that 2 moles of HF are produced for every 2 moles of H and 2 moles of F.

Since we have 2000 moles of H and 2000 moles of F, we will produce 2000 moles of HF.

Now, we can calculate the energy produced using the given information:

2000 moles HF x 500 kJ/mol = 1,000,000 kJ

However, the question asks for the answer in kJ, not kJ/mol. So, we divide by the number of moles (2000) to get the answer in kJ:

1,000,000 kJ / 2000 moles = 500 kJ

Therefore, the energy required for 2 kmol of HF from 2.0kg H and 38 kg F is 500 kJ.

I hope this helps! Let me know if you have any other questions.