Densityof a Gas at

STPLesson # 4

1. Calculate the density of N2 at STP. Calculate

Density = gramslitre

Assume that you

have 1 mole of N2

1. Calculate the density of N2 at STP. Calculate

Density = gramslitre

28.0 g =Assume that you

have 1 mole of N2

1. Calculate the density of N2 at STP. Calculate

Density = gramslitre

28.0 g = 22.4 L

Assume that youhave 1 mole of N2

1. Calculate the density of N2 at STP. Calculate

Density = gramslitre

28.0 g = 1.25 g/L 22.4 L

Assume that youhave 1 mole of N2

2. Calculate the density of CO2 at STP.

Density = gramslitre

Assume that you

have 1 mole of CO2

2. Calculate the density of CO2 at STP. Calculate

Density = gramslitre

44.0 g =Assume that you

have 1 mole of CO2

2. Calculate the density of CO2 at STP. Calculate

Density = gramslitre

44.0 g = 22.4 L

Assume that youhave 1 mole of CO2

2. Calculate the density of CO2 at STP. Calculate

Density = gramslitre

44.0 g = 1.96 g/L 22.4 L

Assume that youhave 1 mole of CO2

3. 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

12.5 g ? L 1

2

3. 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

12.5 g ? L

12.5 g HgO x 1mole216.6g

3. 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

12.5 g ? L

12.5 g HgO x 1mole x 1 mole O2

216.6g 2 mole HgO

3. 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

12.5 g ? L

12.5 g HgO x 1mole x 1 mole O2 x 22.4 L216.6g 2 mole HgO 1 mole

3. 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

12.5 g ? L

12.5 g HgO x 1mole x 1 mole O2 x 22.4 L x 0.450216.6g 2 mole HgO 1 mole

3. 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

12.5 g ? L

12.5 g HgO x 1mole x 1 mole O2 x 22.4 L x 0.450 = 0.291 L216.6g 2 mole HgO 1 mole

4. How many litres of CO2 are produced by the reaction of 100. g of Fe2O3, if the actual yield was 19.0 L @ STP, calculate the percentage yield.

19.0 L2Fe2O3 + 3C 4Fe + 3CO2 100. g ? L3

2

4. How many litres of CO2 are produced by the reaction of 100. g of Fe2O3, if the actual yield was 19.0 L @ STP, calculate the percentage yield.

19.0 L2Fe2O3 + 3C 4Fe + 3CO2 100. g ? L

100. g Fe2O3 x 1 mole x 3 mole CO2 x 22.4 L = 21.05 L 159.6 g 2 mole Fe2O3 1 mole

Percentage yield = 19.0 L x 100% = 90.3 %21.05 L

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