Asked by Bill
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
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
Answers
Answered by
DrBob222
PV = nRT and solve for n = number of mols of H2. In the process one should reduce the total P by vapor pressure of H2O at 25C; however, that information is not included in the problem.
Then n mols H2 = same mols M, then
grams = mols/molar mass. You know grams and mols, solve for molar (atomic) mass M.
Then n mols H2 = same mols M, then
grams = mols/molar mass. You know grams and mols, solve for molar (atomic) mass M.
Answered by
Bill
Is the answer 3.24x10^-3 g/mol?
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.