If ( 1 / 2 ) moles of oxygen combine with Aluminimum to form ( mathrm{Al}_{2} mathrm{O}_{3} ) then weight of Aluminium metal used in the reaction is ( (mathrm{Al}=27)- )
( 4 mathrm{Al}_{(mathrm{s})}+3 mathrm{O}_{2(mathrm{g})} rightarrow 2 mathrm{Al}_{2} mathrm{O}_{3(mathrm{s})} )
(1) ( 27 mathrm{g} )
(2) ( 18 mathrm{g} )
(3) ( 54 mathrm{g} )
(4) ( 40.5 mathrm{g} )

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balanad ( quad lambda_{x n} )
[
4 A l+3 O_{2} rightarrow 2 A L_{2} D_{3}
]
3 molus ob ( 0_{2} ) require 4 molus of Al
0.5 moles of ( 0_{2} )
[
frac{0.5 times 4}{3}=frac{2}{3} text { moles of } mathrm{Al}
]
Mass ob ( frac{2}{3} m o L=frac{2}{3} tan x frac{27 g}{M o L}=18 g )

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