High School
SAT
ACT
University
MCAT
LSAT
DAT

Graham's Law: Kinetic Energy

Related Topics

Wize University Chemistry Textbook > Gases and their Properties

Kinetic Energy, Temperature, and Speed of Gas Particles

6 Activities

Wize University Chemistry Textbook > Gases and their Properties

Graham's Law of Effusion

3 Activities

1. If a mixture of He and Xe are present in a vessel, and the root mean square speed of He is 412 m/s, what is the root mean square speed of Xe? What is the temperature of this vessel?
More Kinetic Energy, Temperature, and Speed of Gas Particles Questions:
Molecular Theory of Gases: Kinetic Energy
Which of the following have the same kinetic energy?
He at 297 K He at 351 K H2 at 297 K O2 at 212 K SO2 at 297 K
Collision theory: Root Mean Square Speed
Which of the following would have the lowest root mean square speed?
a) NO2 at 273 K b) NO2 at 453 K c) O2 at 273 K
Consider the following two curves showing distributions of number of molecules vs. their kinetic energies for two different gas samples. Which of the following statements is not consistent with the two curves?
If the temperature of a sample of an unknown gas is increased from 0 °C to 100 °C, what will be the new root mean square speed of the particles if the original value was 330 m/s?
If a mixture of He and Xe are present in a vessel, and the root mean square speed of He is 412 m/s, what is the root mean square speed of Xe? What is the temperature of this vessel?
Gas Laws
Choose the correct statement(s):
Kinetic Molecular Theory
1. Compare the average kinetic energies of SiH4 and CH4 at a specific temperature?
2. Place these gases in order of increasing average molecular speed at 25 °C: Kr, CH4, N2, CH2Cl2.
Kinetic Molecular Theory
Calculate the ratio of the rms speed of N2 molecules 100 ⁰C to the rms speed of the same at 0 ⁰C.
Kinetic Energy and Temperature
3. If the temperature of a sample of an unknown gas is increased from 0 °C to 100 °C, what will be the new root mean square speed of the particles if the original value was 330 m/s?
How does the root mean square speed of a gas vary with molar mass?
Which of the following have the same kinetic energy?
I He at 297 K
II He at 351 K
Collision theory: Root Mean Square Speed
Which of the following would have the lowest rms?
a) NO2 at 273 K b) NO2 at 453 K c) O2 at 273 K
Molecular Theory of Gases: Kinetic Energy
Which of the following have the same kinetic energy?
He at 297 K He at 351 K H2 at 297 K O2 at 212 K SO2 at 297 K
Molecular theory of gases: Kinetic energy
Which one of the following gases has the greatest average molecular velocity at 300 K?
Atom: Wave-Particle
An proton is confined in a 1-D box with a length of 40 pm.
What is the wavelength of the proton when n = 3?
Atom: Kinetic Energy
An proton is confined in a 1-D box with a length of 40 pm.
What is the kinetic energy of the proton when n = 3?
Atom: Kinetic Energy
A proton is confined in a 1-D box with a length of 40 pm.
Would moving to a larger box result in higher or lower energy?
Kinetic Molecular Theory
Suppose you have a sample of gas at a fixed temperature, and you increase the volume of the container. The pressure changes, since there are...
Gas Laws
Suppose you have a sample of gas at a fixed temperature, and you increase the volume of the container. The pressure changes, since there are...
Kinetic Molecular Theory
Which statement is false?
Consider the following two curves showing distributions of number of molecules vs. their kinetic energies for two different gas samples. Which of the following statements is not consistent with the two curves?
The following curves show the distribution of molecules vs. speed for two different samples of gas, System 1 and System 2. The area under both curves is equal. Which of these descriptions is not consistent with the differences between these two graphs?
More Graham's Law of Effusion Questions:
Graham's Law: Effusion
An ambitious group of scientists conducted two separate experiments where they isolated 1000 atoms each of Li and Rb in a tiny volume of 5 x 10-15 m3 at a temperature of 1 Kelvin. How many times faster or slower would Li atoms be effusing than Rb atoms?
A mixture of Cl2 and Br2 is connected to an empty vessel with a small pinhole. After a long period of time has passed, what will be the ratio of Cl2 to Br2 particles present in the formerly evacuated vessel?
If it takes 24 minutes for a pressure of 20.0 kPa of fluorine gas to accumulate in a vessel through a pinhole, how long will it take for the same pressure to accumulate of H2 gas?
If a mixture of He and Xe are present in a vessel, and the root mean square speed of He is 412 m/s, what is the root mean square speed of Xe? What is the temperature of this vessel?
Nickel forms a gaseous compound of the formulaNi(CO)x{\small \text{Ni(CO)}_\text{x}}. What is the value of x given the fact that under the same conditions of temperature and pressure, methane(CH4){\small \text{(CH}_4)}effuses 3.3 times faster than the compound?
Effusion
One of two identical balloons contained carbon dioxide (CO2) gas and the other contained hydrogen (H2) gas. If it took 24 hours for all of the H2 to effuse out of its balloon, how long did it take for all of the CO2 to effuse?
Graham's Law
2. If it takes 24 minutes for a pressure of 20.0 kPa of fluorine gas to accumulate in a vessel through a pinhole, how long will it take for the same pressure to accumulate of H2 gas?
Graham's Law
4. A mixture of Cl2 and Br2 is connected to an empty vessel with a small pinhole. After a long period of time has passed, what will be the ratio of Cl2 to Br2 particles present in the formerly evacuated vessel?
Gas Laws: Diffusion & Effusion
In the above example, if we started with the same # of dark and light particles and after a certain amount of time passed we looked and saw that there were 4 dark particles and 2 light particles, how much heavier/lighter are the dark particles than the light particles?
If it takes 22.0 minutes for a pressure of 34.0 kPa of neon gas to accumulate in a vessel through a pinhole, how long will it take for the same pressure to accumulate of H2 gas?
Graham's Law
Two gas vessels are linked by a small pinhole which can be opened or closed. When one vessel is evacuated and the other is charged with 100 kPa of F2 gas, it is found that a pressure of 7.42 kPa accumulates in the evacuated vessel after the pinhole has been opened for 15 minutes. If the same experiment was repeated with Cl2 gas, what would the pressure in the evacuated vessel be after 15 minutes? Report your answer in kPa to two decimal places.
A mixture of Cl2 and I2 is connected to an evacuated (empty) vessel with a small pinhole. After an hour has passed, the pin hole is closed. What will be the ratio of Cl2 to I2 particles present in the formerly evacuated vessel?
Effusion
In an effusion experiment, 5.52⋅10−35.52\cdot10^{-3} mols Cl2 was found to effuse through a little orifice in 82 seconds. In another experiment, 4.32⋅10−34.32\cdot10^{-3} mols of an unknown gas effused out under same experimental condition in 47 seconds. Identify the unknown gas.
Graham's Law: Effusion
An ambitious group of scientists conducted two separate experiments where they isolated 1000 atoms each of Li and Rb in a tiny volume of 5 x 10-15 m3 at a temperature of 1 Kelvin. How many times faster or slower would Li atoms be effusing than Rb atoms?