A 0.55 g sample of a certain metal reacted with acid to liberate 375.0 mL of hydrogen gas when collected over water at 20.0 degree Celsius and 790.0 torr (corrected room pressure). The vapor pressure of water is 17.535 mm Hg at this temp. Assuming there is no need to account for pressure differences due to water levels, and using the reaction below, what is the molar mass and identity of the metal? 2X + 6HCl --> 3H2 + 2XCl3

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A 0.55 g sample of a certain metal reacted with acid to liberate 375.0 mL of hydrogen gas when collected over water at 20.0 degree Celsius and 790.0 torr (corrected room pressure). The vapor pressure of water is 17.535 mm Hg at this temp. Assuming there is no need to account for pressure differences due to water levels, and using the reaction below, what is the molar mass and identity of the metal?

2X + 6HCl --> 3H2 + 2XCl3

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