Density of a Gas at STP Lesson # 4.

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Presentation transcript:

Density of a Gas at STP Lesson # 4

1. Calculate the density of N2 at STP. grams Density = litre Assume that you have 1 mole of N2 28.0 g = 1.25 g/L 22.4 L

2. Calculate the density of CO2 at STP. grams Density = litre Assume that you have 1 mole of CO2 44.0 g = 1.96 g/L 22.4 L

3. Calculate the molar mass of gas that weighs 0. 2668 g and has 3. Calculate the molar mass of gas that weighs 0.2668 g and has a STP molar volume of 175.7 mL. If the gas can be found in Harrison Hot Spring water, determine the gas. x 1 L x 1 mol 175.7 mL = 0.0078438 mol 1000 mL 22.4 L grams Molar Mass = mole 0.2668 g Molar Mass = 0.0078438 mol = 34.01 g/mol = H2S

4. Calculate the volume of O2 gas produced at STP for the 4. Calculate the volume of O2 gas produced at STP for the complete decomposition of 12.5 g HgO if the yield is 45.0 %. 2HgO → 2Hg + O2 12 12.5 g ? L 12.5 g HgO x 1mole x 1 mole O2 x 22.4 L x 0.450 = 0.291 L 216.6 g 2 mole HgO 1 mole

5. Calculate the theoretical yield in litres at STP of CO2 in the 5. Calculate the theoretical yield in litres at STP of CO2 in the reaction of 100. g of Fe2O3. If the actual yield was 19.0 L @ STP, calculate the percentage yield. 2Fe2O3 + 3C  4Fe + 3CO2 100. g Fe2O3 x 1 mole x 3 mole CO2 x 22.4 L = 21.0 L 159.6 g 2 mole Fe2O3 1 mole Percentage yield = 19.0 L x 100% = 90.3 % 21.05 L 19.0 L 3 2 100. g ? L