Question

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?

Answer 1

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`