A student performed the experiment as described in the lab manual, using 5.00 mL
ID: 546865 • Letter: A
Question
A student performed the experiment as described in the lab manual, using 5.00 mL of an aqueous hydrogen peroxide solution with a density of 1.01 g/mL. The water temperature was 294 K and the barometric pressure was 31.50 in. Hg. After the student immersed the yeast in the peroxide solution, they observed a 43.34 mL change in system volume as a result of the production of oxygen gas. Use the lab manual to help you solve this question The barometric pressure, in torr, is 800.1 The water vapor pressure at the water temperature is 18.7 The pressure exerted by the collected oxygen gas at the water temperature is 781.4 torr. (1 decimal place) torr. (1 decimal place) torr (1 dec place) or 1.03 atm (2 dec places). The volume of collected oxygen gas is L (4 significant figures). 2 dec places) x 10 Using R-0.08206, the number of moles of collected oxygen gas is 1.85 -3 (integer) mol.Explanation / Answer
Volume of collected oxygen gas = P / nRT = 1.03 / ( 1.85 x 0.08206 x 294 )
Volume of collected oxygen gas = 0.0231 L
Mass of peroxide solution = 1.01 x 5 = 5.05 g
Mass % of peroxide = (0.126 / 5.05) x 100 = 2.495 %
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