13. Consider two containers of volume 1.0 L at 298 K, as shown below.  One container holds 0.10 mol N2 and the other holds 0.10 mol H2.  The average kinetic energy of the nitrogen molecules is 6.2 X 10 -21 J.  Assume that the N2 and the H2 exhibit ideal behavior.   a.   Is the pressure in the container holding the H2 less than, greater than, or equal to the pressure in the container holding the N2.  Justify your answer. b. What is the average kinetic energy of the H2 molecules? c. The molecules of which gas, N2 or H2, have the greater average speed?  Justify your answer. d. What change could be made that would decrease the average kinetic energy of the molecules in the container?

What pressure (in atm) will 0.31 moles of C2H6(g) have at 77.0 °C in a 200.0 mL container? Pressure in atm:

For many purposes we can treat methane (CH,) as an ideal gas at temperatures above Its bolling point of-161. °C. Suppose the temperature of a sample of methane gas is ralsed from -21.0 °C to 13.0 °C, and at the same time the pressure is changed. If the Initlal pressure was 2.8 atm and the volume Increased by 30.0%, what is the final pressure? Round your answer to the correct number of significant digits. atm x10

A. an experiment was done to determine the value of the ideal gas constant( R). hydrogen gas was generated and collected at a given temperature and pressure 1.44X 10 ^-3 moles of hydrogen gas occupied 35.9 mL at 758.0 MMHG and 23.2 Celsius based on these values, calculate the experimentally determine value of R (L x atm/mol x K). B. Using the ungrounded number for the previous problem determine the percent error for the experimentally determined value of R.

7. The partial pressure of CH4(g) is 0.175 atm and that of O2(g) is 0.250 atm in a mixture of the two gases. a. What is the mole fraction of each gas in the mixture? b. If the mixture occupies a volume of 10.5 L at 65°C, calculate the total number of moles of gas in the mixture. C. Calculate the total mass of the mixture (hint, find the mass of each gas in the mixture). с. d. Calculate the relative rates of effusion for molecules of CH4 to that of a molecules of O2.

9)A sample of oxygengas collected at a pressure of 1.05atm and a temperature of 301K is found to occupy a volume of 568milliliters. How many moles of O2gas are in the sample?   Can you show me your work on paper so that I can better understand it?

or many purposes we on treat propane (C₂¹) as an ideal gas at temperatures above its boiling point of -42. °C. Suppose the temperature of a sample of propane gas is lowered from 12.0 °C to -31.0 °C, and at the same time the pressure is increased by 5.0%. Does the volume of the sample increase, decrease, or stay the same? O increase O decrease O stays the same If you said the volume increases or decreases, calculate the percentage change in % the volume. Round your answer to the nearest percent. 0 x10 X

Imagine an ideal gas in a cylinder with a piston, starting at a pressure of 1.00 atm and a volume of 10.0 L at 25.0 °C. This system is cooled to 0.0 °C and compressed to 5.00 L. What is the final pressure in the cylinder, in atm?

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)

1. A 23.1 mL sample of H2 gas was collected from an experiment at 1.079 atm and 22.9  °C. How many moles of gas are in this sample? 2. Suppose you are collecting a gas over water at 23 oC and obtain a pressure reading of 788.3 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? These are two different questions