A0.216 g sample of an aluminium compound x reacts with an excess of water to produce a single hydrocarbon gas. this gas burns completely in o2 to form h2o and co2 only. the volume of co2 at room temperature and pressure is 108cm3 . what is the formula of x

0.216g of aluminium compound X  react with an excess of water water to produce gas. this gas burn completely  in O2  to form H2O and 108cm^3of CO2 only . the volume of CO2 was measured at room temperature and pressure

0.108 / n  =  24 / 1 
n = 0.0045 mole ( CO2 >>0.0045 mole 
0.216 - 0.0045 = 0.2115
so Al =   0.2115 / 27  =>  0.0078 mole 
C = 0.0045 * 1000 => 4.5    and Al  = 0.0078 * 1000 = 7.8 

You need to divided twenty four by a dozen them by the temperature it is getting cook by

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