Gas Stoichiometry & Dalton’s Law of Partial Pressure

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Presentation transcript:

Gas Stoichiometry & Dalton’s Law of Partial Pressure

Example C3H8 + 5O2  3CO2 + 4 H2O What volume of oxygen gas is needed for the complete combustion of 4.00 L C3H8?

Another Example How many g of CaH2 are required to generate 25.0 L of H2 at STP? CaH2 + 2H2O  Ca(OH)2 + 2H2

What if you are NOT at STP? If you are not at STP, you MUST use your equations You MUST look to make sure you are using the right units (including the right gas)

Example N2 + 3H2  2NH3 If 5.00 L of N2 react completely at 3.00 atm and 298 K, how many grams of ammonia are produced?

Dalton’s Law of Partial Pressure The total pressure of a mixture of gases = the sum of the pressures that each gas would exert if present alone. PT = P1 + P2 + P3 +… Also, nT = n1 + n2 + n3 +…

Dalton’s Law of Partial Pressure PTV = (nT)RT P1V = (n1)RT

Example A gaseous mixture is made from 6.00 g O2 and 9.00 g CH4 in a 15.0 L vessel at 273 K. What is the partial pressure of each gas?

Try this example What is the total pressure exerted by a mixture of 2.00 g of hydrogen gas ans 8.00 g of nitrogen gas at 273 K in a 10.0 L vessel?

Collecting Gases Over Water In chemistry it is often necessary to determine the number of moles of a gas generated in a chemical reaction. We do this by water displacement

Total Pressure P T = P gas + P water vapor The pressure of the water vapor can be looked up in a chart in appendix B

Example A sample of KClO3 is partially decomposed producing oxygen gas that is collected over water. The total volume of gas that is collected is 0.250 L at 26°C and 765 torr (1atm = 760 torr) Question #1 How many moles of oxygen were collected?

Example

Question # 2 Calculate the number of grams of KClO3 that were actually decomposed

Another Example NH4NO2  N2 + 2H2O A sample of ammonium nitrite is decomposed and 511 ml of gas are collected over water at 26°C and 745 torr of total pressure. How many grams of ammonium nitrite were decomposed?

Another Example

Diffusion Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing.

Effusion Effusion: describes the passage of gas into an evacuated chamber.

Graham’s Law of Effusion Rate of effusion for gas 1 = √M2 Rate of effusion for gas 2 √M1 Example: Calculate the effusion rates for hydrogen gas (H2) and uranium hexafluoride (UF6)