The oxidation of phosphine (PH3) to phosphorus pentoxide (P2O5) is given by the chemical reaction. __PH3 +__O2 ---> __P2O5 + __H2O b. How many grams of O2 will react completely with 35.0 grams of PH3? c. How many grams of P2O5 and H2O will be produced in the reaction? d. If the reaction give 64% yield. How many grams of PH3 should be used to give an actual yield of 250 grams of P2O5?
The oxidation of phosphine (PH3) to phosphorus pentoxide (P2O5) is given by the chemical reaction. __PH3 +__O2 ---> __P2O5 + __H2O b. How many grams of O2 will react completely with 35.0 grams of PH3? c. How many grams of P2O5 and H2O will be produced in the reaction? d. If the reaction give 64% yield. How many grams of PH3 should be used to give an actual yield of 250 grams of P2O5?
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter4: Stoichiometry Of Chemical Reactions
Section: Chapter Questions
Problem 54E: In an accident, a solution containing 2.5 kg of nitric acid was spilled. Two kilograms of Na2CO3 was...
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The oxidation of phosphine (PH3) to phosphorus pentoxide (P2O5) is given by the
__PH3 +__O2 ---> __P2O5 + __H2O
b. How many grams of O2 will react completely with 35.0 grams of PH3?
c. How many grams of P2O5 and H2O will be produced in the reaction?
d. If the reaction give 64% yield. How many grams of PH3 should be used to give an actual yield of 250 grams of P2O5?
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