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Posted by on Friday, November 7, 2008 at 3:47am.

A 2.91 gram sample of a gaseous compound that contains only boron and hydrogen has a volume of 1.22 L at 25°C and 1.09 atm. What is the formula of this compound? (Atomic Weight: H = 1.01, B = 10.8 amu)

I am not sure but it is B6H10? But I am nto sure if that way i did it anyways was right.

Can someone verify what they get. That would be great

  • chemistry - , Friday, November 7, 2008 at 10:30am

    Use PV = nRT to determine the number of mols, n.
    Then n = g/molar mass will give you the molar mass.
    From there it's guess work unless I've missed something.
    BH3 is the basic compound.
    B2H6
    B4H10
    B5H9
    B5H11
    B6H10
    B10H14
    are the compounds between B and H I can find. Pick the one that comes the closest to the molar mass. Unless I missed the arithmetic I would go with B4H10.
    Check my thinking.

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