Question

Data Collecting hydrogen gas from the reaction of Mg with HCI Trial 1 Trial 2 Trial 3 Atmospheric pressure (in Hg) O pen Mass Mg ribbon 0.069 1.osa. 1.069 Volume Ha collected (ml) sim 40 mL de ML Temperature of water (°C) 23 с әət 1 22oC Vapor pressure of water (Table 10.1) 19.8WHO 19.8 mmHg 1.8 in Ho Atmospheric pressure (mm Hg) Partial pressure of H2 Temperature of water (K) Volume of H: collected (L) Moles Hz Theoretical moles of H: Percent yield Calculations (show for trial 1 only) Balanced chemical reaction with phases: Atmospheric pressure (mmHg Partial pressure House Dalton's Law Generating Hydrogen Gas LAB 10 109

Answer 1

The atmospheric pressure is 760 mmHg.

The partial pressure of H2 is calculated.

P H2 = P atm - P H2O = 760 - 19.8 = 740.2 mmHg

The water temperature in Kelvin is calculated:

T H2O = T ° C + 273 = 22 + 273 = 295 K

The volume is calculated in L:

V = mL / 1000 = 51 mL / 1000 = 0.051 L

Trial 2: 0.046 L

Trial 3: 0.066 L

The moles of H2 are calculated:

n H2 = P * V / R * T = (740.2 / 760) * 0.051 L / 0.082 * 295 = 0.0020 mol

Trial 2: 0.0019 mol

Trial 3: 0.0027 mol

Theoretical moles are calculated:

n H2 = 0.06 g Mg * (1 mol Mg / 24.3 g) = 0.0025 mol

Trial 2: 0.0021 mol

Trial 3: 0.0033 mol

The yield percentage is calculated:

% yield = 0.002 * 100 / 0.0025 = 80%

Trial 2: 90.5%

Trial 3: 81.8%

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