Respuesta :
Answer: 27.1 gram
Explanation:
To calculate the moles :
[tex]\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}[/tex]
[tex]\text{Moles of} P_4=\frac{6.12g}{124g/mol}=0.0494moles[/tex]
The balanced chemical reaction is:
[tex]P_4(s)+6Cl_2(g)\rightarrow 4PCl_3(l)[/tex]
As [tex]Cl_2[/tex] is the excess reagent, [tex]P_4[/tex] is the limiting reagent as it limits the formation of product.
According to stoichiometry :
1 mole of [tex]P_4[/tex] give = 4 moles of [tex]PCL_3[/tex]
Thus 0.0494 moles of [tex]O_2[/tex] give =[tex]\frac{4}{1}\times 0.0494=0.198moles[/tex] of [tex]PCl_3[/tex]
Mass of [tex]PCl_3=moles\times {\text {Molar mass}}=0.198moles\times 137g/mol=27.1g[/tex]
Thus 27.1 g is the theoretical yield of phosphorus trichloride
