Post a New Question

Chemistry

posted by on .

A 0.528 gram sample of a metal, M, reacts completely with sulfuric acid according to: M+H2SO4 -> MSO4+H2

A volume of 205 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.

? g/mol

Is the answer 3.24x10^-3 g/mol?

  • Chemistry - ,

    No. If you will show your work I will look for the error. I think I answered this for you yesterday. I used as pressure of Ptotal = 756 mm + pH2O
    and a table gave 23.8 mm for vapor pressure of H2O at 25C.

  • Chemistry - ,

    n=.0833 mols
    molar mass=(.0833mols/.528g)=.158g/mol

  • Chemistry - ,

    What did you substitute for PV = nRT?

  • Chemistry - ,

    P=.995atm
    V=.205L
    n=?
    R=.0821 Lxatm/molxk)
    T=298K

  • Chemistry - ,

    It is 65.4g/mol

  • Chemistry - ,

    I would use P = (756-23.8)/760 = 0.963 atm; however, going with your number will still get close to the right answer.
    PV = nRT or
    n = PV/RT = 0.995*0.205/0.8206*298
    n = 0.00834. You had to use some other (incorrect) version of n = PV/RT.
    Then n = grams/molar mass or
    molar mass = grams/n
    molar mass = 0.528.0.00834 = ?
    If you use P = (756-23.8)/760 I think you will get 65.4 which is Zn.

Answer This Question

First Name:
School Subject:
Answer:

Related Questions

More Related Questions

Post a New Question