A 0.504 gram sample of a metal, M, reacts completely with sulfuric acid accordin
ID: 897382 • Letter: A
Question
A 0.504 gram sample of a metal, M, reacts completely with sulfuric acid according to: M(s) + H2SO4 (aq) = MSO (aq) + H2 (g) A volume of 233 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 molar mass of the metal. I used the same formulas that I saw on other questions similar to this one, but got answers 52.6 and 51.0. Neither answer was correct. I must be doing something wrong but I can't figure out what exactly. Help please!
Explanation / Answer
PV = nRT
PV = Wt/Mwt * RT
Mwt = Wt / PV * RT
= 0.504 * 298 * 82.1/ 0.994atm * 233ml
= 53.2 molar mass
your answer was also correct
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