Asked by Jeff
Consider the following unbalanced reaction.
P4(s) + F2(g)---> PF3(g)
How many grams of F2 are needed to produce 114 g of PF3 if the reaction has a 80.3% yield?
I've worked it every way I can think, and the online grader says I am wrong. Someone plz lend me a hand.
P4(s) + F2(g)---> PF3(g)
How many grams of F2 are needed to produce 114 g of PF3 if the reaction has a 80.3% yield?
I've worked it every way I can think, and the online grader says I am wrong. Someone plz lend me a hand.
Answers
Answered by
bobpursley
well, there are about 50 ways to do it.
114 g of PF3 has how many grams of F in it? 114*atomicmassF/molmassPF3= 114(31/(50)=? you can work all that more accurately.
so how many grams of F2 is this? answer: 1/2 of the above.
With 80.3 percent yield? you need aboveF2 mass* (1/.803) grams F2
114 g of PF3 has how many grams of F in it? 114*atomicmassF/molmassPF3= 114(31/(50)=? you can work all that more accurately.
so how many grams of F2 is this? answer: 1/2 of the above.
With 80.3 percent yield? you need aboveF2 mass* (1/.803) grams F2
Answered by
bobpursley
The conventional way to do this is with mole ratios, but it has to be balanced first.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.