How do you balance #PH_3 + O_2 -> P_4O_10 + H_2O#?

1 Answer
Mar 5, 2016

Answer:

You balance this redox equation stoichiometrically.

Explanation:

#4PH_3(g) + 8O_2(g) rarr P_4O_10(s) + 6H_2O(l)#

IS this equation stoichiometrically balanced; that is for every reactant particle, is there a corresponding product particle?

Combustion reactions like these can usually be balanced directly, without that tedious mucking about with redox half equations. Hydrocarbon combustion reactions might be balanced the same way. Note that this IS FORMALLY a redox reaction: #P(-III)# is oxidized to #P(+V)#. What is reduced here?