In the reaction #P_4 + 5O_2 -> PO_4O_10#, 7.75 g #P_4# reacts. How do you calculate the mass of #P_4O_10# produced?

1 Answer
Mar 3, 2017

Answer:

We follow the stoichiometric equation..........and get approx. #4*g#.

Explanation:

#P_4(s) + 5O_2(g) rarr P_4O_10(s)#

#P^(0)# is oxidized up to #P^(V)#.

#"Moles of white phosphorus:"#

#=# #(7.75*g)/(4xx30.9737*g*mol^-1)=6.26xx10^-2*mol.#

And thus, given excess dioxygen (reasonable!), we can calculate the mass of oxide as:

#1/4xx6.26xx10^-2*molxx283.89*g*mol^-1=??g#