0.144 g of an aluminium compound X react with an excess of water to produce a gas. This gas burns completely in O2 to form H2O and 72cm3 of CO2 only. Volume of CO2 was measured at room temperature and pressure. Deduce the formula of X
X - AlxCy; AlxCy + H2O = Al(OH)3↓ + CH4↑; CH4 + 2O2 = CO2 + 2H2O; ν(CH4) = 0.072/22.4 = 0.0032mol; Because the valence of Al is 3, and the valence of C is 4 and z is taken as coefficient of proportionality, then Μ(AlxCy) = 26*4z+12*3z; We have the next equation: 0.0032/3 = 0.144/26*4z + 12*3z; 0.001 = 0.144/140z; z=1. So, formula of X is Al4C3.
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