A 0.464 gram sample of a metal, M, reacts completely with sulfuric acid according to:
M(s) +H2SO4(aq)=MSO4(aq)+H2(g)
A volume of 211 mL of hydrogen is collected over water; the water level in the collecting vessel is the same as the outside level. Atmospheric pressure is 756.0 Torr and the temperature is 25°C. Calculate the atomic mass of the metal. Every time it's wrong. Please walk me through this

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  1. R=62.3637 L·Torr/mol·K
    P=756.0 Torr

    Use PV=nRT and solve for moles, n.

    moles of H2=n=PV/RT

    moles of H2=moles of M

    You know that

    moles of M=0.464g of M


    1 mole of M=Atomic weight

    (moles of M/0.464g of M)=(1 mole of M/Atomic weight)

    solve for atomic weight,

    atomic weight=0.464g of M/moles of M

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  2. I think there must be a correction for the vapor pressure of H2O at the temperature stated.
    That would make that part
    (756-23.8)(0.211)/[(62.364*298)]= 0.00831 mols. Then proceed to molar mass.

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  3. Okay, I think I see why.

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