Question

PRE-LAB QUESTIONS 1. A student did the experiment described except she used Al foil instead of Mg. Her data table included the following values. Mass of Al 0.0352 g Temperature 19.08 °C Barometric pressure 762.5 mm Hg Volume of H, gas 46.92 mL Answer the following questions based on this data table. a, Write the balanced equation for the reaction between Aluminum and hydrochloric acid. a Al tHCI AIC t3 b. How many moles of Al were consumed? A1-36.989/mot Hnsamed O, 03 5L molg 36.98 -3 = 1.30 X10moe c. How many moles of H, were produced? Al 3H =L.30X /0-X -195 K10moes H produced d. What was the vapor pressure of the water in the gas sample? (V4.9 mL (El1.ora H2= vbter 625-F59ai m 44.9 03L 1.957 X103 x.ol2 y ad 08 ART -.9989atm a 59.21 MM 3, 289

Answer 1

e) The water vapor pressure is given at the given temperature of 16.5 mmHg, the dry H2 pressure is calculated:

P H2 = 762.5 - 16.5 = 746 mmHg

f) The experimental value of R is calculated:

R = P * V / n * T = (746/760) * 0.04692 / 1.3x10 ^ -3 * (19.08 + 273) = 0.121 atm * L / mol * K

g) The volume is calculated at STP:

V = n * R * T / P = 1.3x10 ^ -3 * 0.121 * 273 K / 1 atm = 0.043 L

h) The molar volume is calculated:

Vm = V / m = 0.043 L / 1.3x10 ^ -3 mol = 33.08 L / mol

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