Question

Use the following balanced reaction to solve:

P4 (s) + 6H2 (g) → 4PH3 (g)

How many grams of phosphorus trihydride will be formed by reacting 60 L of Hydrogen gas with an excess of P4?

Answer 1

Answer: 60.7 g of
`PH_3` will be formed.

Step-by-step explanation:

To calculate the moles :

`\text{Moles of solute}=\frac{\text{given volume}}{\text{Molar volume}}`

`\text{Moles of} H_2=(60L)/(22.4L)=2.68moles`

The balanced chemical reaction is

`P_4(s)+6H_2(g)\rightarrow 4PH_3(g)`

`H_2` is the limiting reagent as it limits the formation of product and
`P_4` is the excess reagent.

According to stoichiometry :

6 moles of
`H_2` produce = 4 moles of
`PH_3`

Thus 2.68 moles of
`H_2` will produce=
`(4)/(6)* 2.68=1.79moles` of
`PH_3`

Mass of
`PH_3=moles* {\text {Molar mass}}=1.79moles* 33.9g/mol=60.7g`

Thus 60.7 g of
`PH_3` will be formed by reactiong 60 L of hydrogen gas with an excess of
`P_4`