Asked by Engelbert
The oxidation of phosphine (PH3) to phosphorus pentoxide (P2O5) is given by the chemical equation:
_PH3+O2-->_P2O5+H2O
A.balance the chemical equation
B.how many grams of O2 will react completely with 35.0grams of PH3?
C.how many of P2O5 and H2O will be produced in the reaction?
D.if the reaction gives 64% yield,how many grams of PH3 should be used to produce an actual yield of 250grams of P2O5?
_PH3+O2-->_P2O5+H2O
A.balance the chemical equation
B.how many grams of O2 will react completely with 35.0grams of PH3?
C.how many of P2O5 and H2O will be produced in the reaction?
D.if the reaction gives 64% yield,how many grams of PH3 should be used to produce an actual yield of 250grams of P2O5?
Answers
Answered by
bobpursley
go thru this similar problem (answer is on second page). Then try this one, I will be happy to check your work. http://www.wou.edu/las/physci/poston/ch221/pdf/Limiting-Reagent-Problems-Key.pdf
Answered by
Anonymous
D. 76.62 g
Answered by
Unidentified
Where can i get the answer? Help please
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