Four 0.6 mol samples of xenon gas are described in the table below. Rank these samples in order of decreasing rate of collisions between atoms. That is, select "1" next to the sample with the most collisions per second between Xe atoms and the walls of the container. Select "2" next to the sample with the next most collisions per second between Xe atoms and the walls of the container, and so on. sample A B C D volume 27. L 21 L 31 L 21. L temperature -95 °C 69. C -95 °C -95 °C X collisions per second 1 (most) 2 3 4 (least)

Four 0.6 mol samples of xenon gas are described in the table below. Rank these samples in order of decreasing rate of collisions between atoms. That is, select "1" next to the sample with the most collisions per second between Xe atoms and the walls of the container. Select "2" next to the sample with the next most collisions per second between Xe atoms and the walls of the container, and so on. sample A B C D volume 27. L 21 L 31 L 21. L temperature -95 °C 69. C -95 °C -95 °C X collisions per second 1 (most) 2 3 4 (least)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Four 0.9 mol samples of krypton gas are described in the table below. Rank these samples in order of decreasing rate of collisions between atoms. That is, select "1" next to the sample with the most collisions per second between Kr atoms and the walls of the container. Select "2" next to the sample with the next most collisions per second between Kr atoms and the walls of the container, and so on. collisions per sample volume temperature second A 18. L - 80. °C |(Choose one) ♥ В 24. L - 80. °C |(Choose one) v 21. L -80. °C (Choose one) 18. L -67. °C |(Choose one)
A sample of xenon gas occupies a volume of 7.59 L at 499 K. If the pressure remains constant, at what temperature will this same xenon gas sample have a volume of 4.41 L?
= 630. Consider the arrangement of bulbs shown in the drawing. Each of the bulbs contains a volume of gas as shown. PN₂ torr, PNe = 228 torr, and PH₂ = 448 torr. What is the pressure of the system when all the stopcocks are opened, assuming that the temperature remains constant? (We can neglect the volume of the capillary tubing connecting the bulbs.) 605.31 X torr Volume N₂ 1.0 L Ne 1.0 L H₂ 0.5 L
12. A piece of sodium (Na) metal reacts completely with water to produce NaOH(aq) and H₂(g). The H₂(g) generated is collected over water at 25.0°C. (Vapor pressure of water at 25°C is 0.0313 atm) The volume of the gas is 246 mL measured at normal atmospheric pressure. Calculate the mass (in grams) of Na (MM = 22.99) used in the reaction. 13. Ammonia (NH₁) burns in oxygen gas to form nitric oxide (NO) and water vapor. How many liters of oxygen will react with 8.00 L of ammonia at the same temperature and pressure?
A sample of xenon gas occupies a volume of 7.36 L at 403 K. If the pressure remains constant, at what temperature will this same xenon gas sample have a volume of 4.18 L?
Which statement is TRUE according to the kinetic molecular theory? Which statement is TRUE according to the kinetic molecular theory? A single particle does not move in a straight line. The collisions of particles with one another is not completely elastic. The average kinetic energy of a particle is proportional to the temperature in Kelvin. The size of the particle is large compared to the volume.
The pressure of a sample of argon gas was increased from 3.73 atm to 8.57 atm at constant temperature. If the final volume of the argon sample was 16.9 L, what was the initial volume of the argon sample? Assume ideal behavior.
A student obtained a mass of 0.266 g CO2 during his experiment. The atmospheric pressure was 751.6 mmHg and the laboratory temperature was 24.1 °C. The flask used in the experiment had a volume of 146.5 mL. Calculate the molar mass of CO2 from the data. Hint: You cannot use the molar mass of CO2 in your calculation since this is what you are looking for... You need to used the ideal gas law to determine the number of moles of CO2, then do the ratio of grams of CO2 over moles of CO2 to determine the experimental molar mass of CO2.
73. A 500.-mL sample of O2 gas at 24 °C was prepared by decomposing a 3% aqueous solution of hydrogen peroxide, H2 O2, in the presence of a small amount of manganese catalyst by the reaction 2H2 O2 (aq) → 2H2O (g) + The oxygen thus prepared was collected by displacement of water. The total pressure of gas collected was 755 mm Hg. What is the partial pressure of O2 in the mixture? How many moles of O2 are in the mixture? (The vapor pressure of water at 24 °C is 23 mm Hg.)
4. A glass container was initially charged with 2.00 moles of a gas sample at 3.75 atm and 21.7 °C. Some of the gas was released as the temperature was increased to 28.1 °C, so the final pressure in the container was reduced to 0.998 atm. Assume the volume stayed the same. How many moles of the gas sample are present at the end?
The pressure of a sample of argon gas was increased from 1.57 atm to 6.41 atm at constant temperature. If the final volume of the argon sample was 14.3 L, what was the initial volume of the argon sample? Assume ideal behavior. L