Calculating F2 Needed to Produce 120 g of PF3

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SUMMARY

The discussion centers on calculating the amount of F2 required to produce 120 grams of PF3 in an unbalanced chemical reaction. The participant initially attempted to find the moles of F2 needed by dividing the target mass of PF3 by its molar mass and adjusting for an 84.6% yield, resulting in 1.612 moles. However, the calculation was incorrect due to the oversight of not balancing the chemical equation before proceeding with the stoichiometric calculations. The correct approach requires balancing the reaction before determining the required moles of F2.

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  • Ability to balance chemical equations
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Chemistry students, educators, and anyone involved in chemical calculations or reaction yield assessments will benefit from this discussion.

Pengwuino
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Ok so this problem pissed me off to no end... basically because ih ad 5 minutes to do it and couldn't figure it out.

Consider the following unbalanced reaction:

P4(s) + F2(g) -----> PF3(g)

How many grams of F2 are needed to produce 120. g of PF3 if the reaction has a 84.6 % yield?

Now, i divided the 120g by the molar mass of PF3 and divided by .846 to find the actual amount necessary which gave me 1.612449659 moles. Multply that by the molar mass of F2 and i get 61.26663726. Wasn't correct, wasn't even a matter of significant figures... what went wrong here :D
 
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Did you remember to balance the equation?
 
oh damn it. They were constantly giving me pre-balanced equations and having to do this so i never noticed that they gave me an unbalanced equation...
 
It says it right there jackass :wink:
 

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