Some metals will react with hydrochloric acid to liberate hydrogen gas. The general equation for this reaction is: 2 M(s) + 2x HCl(aq) → 2 MCI×(aq) + x H2(g), where x = 1, 2, or 3. In an experiment to determine the molar mass, and therefore the identity, of a reactive metal, a 0.216 g sample of the metal was combined with an excess of 2.0 M HCl(aq). All of the metal was consumed and the hydrogen gas was collected at a pressure of 760 mmHg in a 150 mL vessel at a temperature of 20 °C. If x = 3, what is the metal? (R = 0.08206 atm-L/mol·K; 0 °C = 273 K; 1 atm = 760 mmHg). Give the full name of the element (all letters lower case).
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Please answer and explain the following
The balanced reaction taking place is given as (for x = 3),
=> 2 M (s) + 6 HCl (aq) --------> 2 MCl3 (aq) + 3 H2 (g)
Given : Mass of metal reacted = 0.216 g
Volume of vessel = 150 mL = 0.150 L (Since 1 L = 1000 mL)
Temperature = 20 oC
And pressure of H2 produced = 760 mm Hg = 1 atm.
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