Question

Station 2: Calculations with the Ideal Gas Law A Station Letter: A student reacted a strip of magnesium metal with 4.00 mL of 4.0 M hydrochloric acid and collected the hydrogen gas produced using the experimental setup you see at the station. Unfortunately, the student forgot to record the mass of the metal before they reacted it with acid. Determine the mass of the magnesium metal the student used in the experiment. For this experiment assume the pressure of the gas in the collection tube is equal to the atmospheric pressure, making it unnecessary to use a leveling tank. The barometric (total) pressure at the time the experiment was conducted was 750.1 mm Hg and the temperature of the water was 25'C. The ideal gas constant is 0.08206 am Make mot-K sure to show all calculations. 7 50.1 Corrected Pressure of Ha in mm Hg Temperature of Water ("C) Pressure (mm Hg) 17.5 18.7 20 4.00mL 21 22 Volume of H2 in mL 19.8 21.1 22.4 23 24 25 26 27 28 Number of mole of Hz 23.8 25.2 26.7 28.3 30.0 31.8 Balanced Chemical Equation for the Reaction 29 30 Mass of Mg Calculations:

Answer 1

Pressure corrected:

P H2 = P total - P H2O = 750.1 - 23.8 = 726.3 mmHg

H2 volume: 4 mL

H2 Moles:

n H2 = P * V / R * T = (726.3 / 760) * 0.004 L / 0.082 * 298 = 1.6x10 ^ -4 mol

The balanced chemical reaction is:

Mg + 2 HCl = MgCl2 + H2

Mg mass is calculated:

m Mg = 1.6x10 ^ -4 mol H2 * (1 mol Mg / 1 mol H2) * (24.3 g Mg / 1 mol) = 0.004 g

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