Check all correct statements about atmospheric pressure P atm gradually decreases as altitude increases Patm is the pressure exerted by the weight of the atmosphere O Liquids boil when the Patm = P vapor P atm is the same regardless of the altitude

A 12.4 L gas cylinder contains 7.44 g He at 17.6 °C. What is the pressure inside the cylinder? (R = 0.08206 L×atm/mol×K) %3D O 3.58 atm 0.217 atm O 14.3 atm 550 atm O 1.03 atm

The total pressure exerted by a mixture of nitrogen, oxygen and water vapor is 742 mmHg in a sealed container. The partial pressure of N2 is 581 mmHg, and the partial pressure of water vapor is 18 mmHg. What is the pressure in atm of the O2 in the container? Note: 760 mmHg = 1 atm

What is the answer for question 8?

A sample of O2 gas was collected over water at a total pressure of 620 mm Hg and 25 degrees c.  The vapor pressure of water at 25 degrees c is 23.8 mm Hg  what is the pressure of O2??

At 298 K, a 5.0-L flask contains 0.15 mol of O2 and 0.22 mol of N2. Calculate the partial pressure of N2 inside the container. (Note: the ideal gas constant is 0.0821 L•atm/mol•K)

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Question #2 I couldn't take a single picture

Suppose you are collecting a gas over water at 23 oC and obtain a pressure reading of 790.2 mm Hg.If the vapor pressure of water is 21.1 mm Hg at the collection temperature, what is the pressure of the collected gas

The height of Mt. Everest is 29,000' and the atmospheric pressure is 253 mmHg (0.333 atm). The gas constant R is 8.314J/K*mol and the heat of vaporization of water (AHvap) is 40.8 kJ/mol. The pressure at sea level is 760 mmHg. Note 1: The P₁ is the pressure at sea level and P₂ is the pressure on Mt. Everest. Note 2: The T₁ temperature is the boiling point of water at sea level which is 100 °C or 373 K. Note 3: The term AHvap is express in kJ/mol. This must be converted to J/mol. a) Using the two component Clausius-Clapeyron equation, determine the boiling point of water on the top of Mt. Everest. InP1/P₂= AHvap/R(1/T2-1/T1) 4