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    A 0.216 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?

    A. Al2C3 B. Al3C2 C. Al3C4 D. Al4C3

    Please help me with this question. Answer scheme says it's D.
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    What have you tried, so far?
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    (Original post by Pigster)
    What have you tried, so far?
    I tried using the general combustion equation but can't seem to get it. Can you please show me the working?
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    How many mol of C atoms are there in the 0.216 g of X?
 
 
 
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