Composition of Dry Air at Sea Level Gas Mole% N2 78.084 O2 20.946 Ar   0.934 CO2   0.0345 Ne   0.00182 He   0.000524 CH4   0.000168 Kr   0.000114 A) Using data from the above table, calculate the partial pressure of Kr when the atmospheric pressure is 1.07 atm. My answer: 1.22×10-6 atm B) At the same atmospheric pressure, if the temperature is 22°C, how many Kr atoms would there be in 310 mL?

Answer part a and b

In a 3-gas system, there are 6.4 kPa Ne, 0.13 atm of He,'and an unknown partial pressure of Ar. If the total pressure was 44.8 kPa, what was the partial pressure of argon in the system (in kPa)? O A. 63.4 ов. 93.3 ос. 10.4 D. 46.7 O E. 25.6 m

A 3.0L sample of gas at 1.0 atm and 0.0℃ is heated to 85℃. Calculate the final volume. The pressure remains constant.

Calculate the mass

The van der Waals equation of state was designed (by Dutch physicist Johannes van der Waals) to predict the relationship between pressure p, volume V and temperature T for gases better than the Ideal Gas Law does: p+a n #2²7) (V- (V-nb)=nRT The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. What are the units of a? The van der Waals equation of state. R stands for the gas constant and n for moles of gas. What are the units of b? For water the numerical value of a is 5.464 and the numerical value of b is 0.0305. Use the van der Waals equation to calculate the pressure of a sample of water at 430.0 °C with a molar volume of 1.92 L/mol. Round your answer to the correct number of significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round your answer to the correct number of significant digits. 1 0 П atm atm x10 H X ロ・ロ S

Consider the lungs, which can be modeled on a very basic level as a 5.0 L container of a mixture of N2 and O2 gases at 298 K. a) Calculate the pressure inside your lungs if filled with 0.15 mol the gas mixture described above, assuming it behaves ideally. b) Is it reasonable to assume that this gas mixture behaves ideally under these conditions? Why or why not?

Vol 752mL Gas X  (g) 2.49g 1.98 atm 62oC     Identity of the gas - by formula ?

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