R=62.3637 L·Torr/mol·K
L=0.211L
P=756.0 Torr
T=273.15+25ºC
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
and
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
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
3 answers
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.
That would make that part
(756-23.8)(0.211)/[(62.364*298)]= 0.00831 mols. Then proceed to molar mass.
Okay, I think I see why.