Question

What is the mole ratio needed to determine the mass of phosphorus trifluoride produced from the reaction of 120 g of phosphorus with excess fluorine?

Answer 1

`(4molPF_3)/(1molP_4)`

Step-by-step explanation:

Hello

In this case, given the reaction:

`P_4(s)+6F_2(g)\rightarrow 4PF_3(g)`

It means that since the coefficients preceding phosphorous and phosphorous trifluoride are 1 and 4, the correct mole ratio should be:

`(4molPF_3)/(1molP_4)`

Because given the mass of phosphorous it is convenient to convert it to moles and then cancel it out with the moles on bottom of the mole ratio.

Bes regards!