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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: magnus on February 09, 2019, 03:09:49 AM

Title: yield %
Post by: magnus on February 09, 2019, 03:09:49 AM

Hi,
from the reaction of 3 moles of fluorine (F₂) with 5 moles of hydrogen (H₂), 5.82 moles of HF
H₂ + F₂ -> 2HF

the stechimetric ratio is 1:1, and the limiting element is F₂.
The yield should be 58%  ???

Title: Re: yield %
Post by: AWK on February 09, 2019, 03:36:10 AM

How many moles of HF you can obtain from 3 moles of F₂?

Title: Re: yield %
Post by: magnus on February 09, 2019, 03:39:10 AM

5.82 moles

Title: Re: yield %
Post by: AWK on February 09, 2019, 03:40:02 AM

This is the real yield. I asked for the theoretical one. So the yield is ...?

Title: Re: yield %
Post by: AWK on February 09, 2019, 04:00:08 AM

Sometimes we ask for the yield in reference to the specified reagent. But this should be clearly stated.

Title: Re: yield %
Post by: magnus on February 09, 2019, 04:07:13 AM

Quote from: AWK on February 09, 2019, 03:40:02 AM

This is the real yield. I asked for the theoretical one. So the yield is ...?

14.55

Title: Re: yield %
Post by: AWK on February 09, 2019, 04:11:14 AM

?
5H₂ + 3F₂ -> ?HF

Title: Re: yield %
Post by: magnus on February 09, 2019, 04:18:09 AM

3 moles of H₂ react with 3 moles of F₂ -> 6 moles HF according to the stoichiometric ratio

H₂ + F₂ -> 2HF

Title: Re: yield %
Post by: AWK on February 09, 2019, 04:20:37 AM

This is a theoretical yield.

Title: Re: yield %
Post by: magnus on February 09, 2019, 04:30:03 AM

5.82/6 * 100= 97%

Title: Re: yield %
Post by: AWK on February 09, 2019, 04:31:10 AM

Solved.

Title: Re: yield %
Post by: magnus on February 09, 2019, 04:48:07 AM

Thanks