Question

For the following reaction, 6.12 grams of phosphorus (P4) are mixed with excess chlorine gas . The reaction yields 21.5 grams of phosphorus trichloride . phosphorus (P4) ( s ) chlorine ( g ) phosphorus trichloride ( l ) What is the theoretical yield of phosphorus trichloride

Answer 1

Answer: 27.1 gram

Step-by-step explanation:

To calculate the moles :

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

`\text{Moles of} P_4=(6.12g)/(124g/mol)=0.0494moles`

The balanced chemical reaction is:

`P_4(s)+6Cl_2(g)\rightarrow 4PCl_3(l)`

As
`Cl_2` is the excess reagent,
`P_4` is the limiting reagent as it limits the formation of product.

According to stoichiometry :

1 mole of
`P_4` give = 4 moles of
`PCL_3`

Thus 0.0494 moles of
`O_2` give =
`(4)/(1)* 0.0494=0.198moles` of
`PCl_3`

Mass of
`PCl_3=moles* {\text {Molar mass}}=0.198moles* 137g/mol=27.1g`

Thus 27.1 g is the theoretical yield of phosphorus trichloride