chapter_10_gases_11dec2017.notebook December 11, 2017
10.5: Gas Density & Molar Mass d=m/V PV = nRTà n/V = P/RT – n x molar mass = mass in grams – d= Pxmolar mass/RT • SO…can solve for density using the ideal gas law • What is the density of carbon tetrachloride vapor at 714 torr and 125oC? chapter_10_gases_11dec2017.notebook December 11, 2017
10.5: Gas Density and Molar Mass
The mean molar mass of the atmosphere at the surface of Titan (Saturn’s largest moon) is 28.6g/mol. The surface temperature is 95K and the pressure is 1.6atm. Assuming ideal behavior, calculate the density of Titan’s atmosphere. chapter_10_gases_11dec2017.notebook December 11, 2017
10.5: Gas Density and Molar Mass A large evacuated flask initially has a mass of 134.567g. When the flask is filled with a gas of unknown molar mass to a pressure of 735 torr at 31C, its mass is 137.456g. When the flask is evacuated again and filled with water at 31C, its mass is 1067.9g. The density of water at this temperature is 0.997g/mL. Assuming the ideal gas equation applies, calculate the molar mass of the gas. chapter_10_gases_11dec2017.notebook December 11, 2017
10.5: Gas Density and Molar Mass Calculate the average molar mass of dry air if it has a density of 1.17g/L at 21C and 740.0 torr. chapter_10_gases_11dec2017.notebook December 11, 2017
10.5: Volume of Gases in Chemical Reactions Coefficients in balanced chemical equation gives the relative amount (moles) of reactants and products Ideal gas equation relates moles to P, V, T Automobile air bags are inflated by nitrogen gas generated by the rapid decomposition of sodium azide (NaN3). If an air bag has a volume of 36L and is to be filled with nitrogen gas at 1.15atm and 26.0oC, how many grams of sodium azide must be decomposed?
In the first step in the industrial process for making nitric acid, ammonia reacts with oxygen in the presence of a suitable catalyst to form nitric oxide (NO) and water vapor. How many liters of ammonia at 850oC and 5.00 atm are required to react with 1.00mol of oxygen in this reaction? chapter_10_gases_11dec2017.notebook December 11, 2017
10.6: Gas Mixtures and Partial Pressure Dalton’s Law of Partial Pressure: the total pressure of a mixture of gases is equal to the sum of the individual pressures of the gases partial pressure: pressure exerted by an individual gas in a mixture of gases PT = PA+ PB + PC+…
How is the pressure exerted by N2 gas affected when some O2 gas is introduced into a container if the temperature and volume remain constant?
Looking at PV= nRT, at constant V&T, the pressure of a gas is determined by the moles of gas mole fraction: ratio of moles of part of the mixture to the total moles in the mixture XA =nA/nT PA = XAxPT What is the pressure of oxygen gas if a mixture contains 4 moles oxygen, 2 moles nitrogen and 2 moles of carbon dioxide. The total pressure is 1.00 atm.
A mixture of 6.00g O2(g) and 9.00g CH4(g) is placed in a 15.0L vessel at 0C. What is the partial pressure of each gas and what is the total pressure in the vessel?
Air is 72% N2 (the mole fraction would be 0.72). What is the partial pressure of N2 if the barometric pressure is 760torr?
because N2 is 72% of the mixture, it contributes 72% of the total pressure