Aluminium reacts with sulphure to form a aluminium sulphide . If 5.4 gm of Aluminium reacts with 12.8 gm sulphure gives 12 gm of aluminium sulphides , then the percent yield of the reaction is-

Explanation

`2Al + 2S to Al_(2)S_(3)`
Mole taken `{:((5.4)/(27) gm ,(12.8)/(32)),(=0.2,=0.4):}`
`("mole taken")/("stoich coeff"){:((0.2)/(2),(0.4)/(3)),(=0.1,=0.133),((L.R.),):}`
moles of `Al_(2)S_(3)` formed `=(1)/(2)xx0.2=0.1`
mass=`0.1xx150=15` gm
`%` yield `=("actual yield")/("theoritical yield")xx100=(12)/(15)xx100=80%`