Question
When 0.422 g of phosphorus is burned, 0.967 g of a white oxide (a compound of phosphorus and oxygen) is obtained.
a. Determine the empirical formula of the oxide.
So for the empirical Formula I got P_2O_5 now it wants me to Write a balanced equation for the reaction of phosphorus and molecular oxygen based on this empirical formula (include states of matter).
I got 4P(s) + 5O2(g) → 2P2O5(s) I don't think this is right can someone please check my work and let me know? Thank you so much!
a. Determine the empirical formula of the oxide.
So for the empirical Formula I got P_2O_5 now it wants me to Write a balanced equation for the reaction of phosphorus and molecular oxygen based on this empirical formula (include states of matter).
I got 4P(s) + 5O2(g) → 2P2O5(s) I don't think this is right can someone please check my work and let me know? Thank you so much!
Answers
Graham
P: 30.973762(2)
O: 15.999(4)
Ratio of O to P is:
((0.967-0.422)/0.422)*(30.973762/15.999) = 2.50
The empirical formula is correctly derived from the given masses.
The empirical equation also balances.
O: 15.999(4)
Ratio of O to P is:
((0.967-0.422)/0.422)*(30.973762/15.999) = 2.50
The empirical formula is correctly derived from the given masses.
The empirical equation also balances.