A 0.566 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H₂SO4 (aq) MSO4 (aq) + H₂(g) A volume of 257 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. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal. -

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Chapter1: Chemical Foundations
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A 0.566 g sample of a metal, M, reacts completely with sulfuric acid according to
M(s) + H₂SO4 (aq) → MSO₂(aq) + H₂(g)
A volume of 257 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. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate
the molar mass of the metal.
Transcribed Image Text:presented by Macmillan Learning A 0.566 g sample of a metal, M, reacts completely with sulfuric acid according to M(s) + H₂SO4 (aq) → MSO₂(aq) + H₂(g) A volume of 257 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. The vapor pressure of water at 25 °C is 23.8 Torr. Calculate the molar mass of the metal.
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