Question

132 PROPOS22: Determining the Molar Mass of Co2 e) Determine the mass of air displaced by the inflated balloorn (0 Determine the measured mass of the CO2 in the balloon. (g) Determine the actual mass of the CO2 in the balloon. (h) Determine the molar mass of Co, () Determine the percent error in your calculated molar mass for CO2, based on the theoretical value of 44.01 g/mol.

Answer 1

Barometric pressure = 28.96 in Hg = 28.96 in Hg times 1 atm/29.92 in H/g = 0.968 atm Laboratory temperature = 22 degree c the relationship between kelvin & calcium scale of the pervasive TK = (degree c + 273) therefore TK = (22 + 273) k = 295 k therefore temperature 295 kelvin volume of balloon = 1730 mL = 1730 mL times 12/10^3 mL [because 1 L = 10^3 mL] = 1.730 L therefore volume of balloon 1.730 liter \r\n using pv = n R t [where, p = pressure = 0.968 atm v = volume = 1.730 L n = Number of mol = ? R = gas constant = 0.08 mL atm mol^-1 k^-1 T = temp = 295 k] therefore 0.968 atm times 1730 L = n times 0.08 L times k atm mol^-1 k^-n times 295 k therefore n = 0.968 times 1730/0.0821 times 295 mol