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Kinetic Molecular Theory - Answer Keys
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- What are the postulates of the kinetic molecular theory? 1. Particles are assumes to have a V = 0 2. Particles are in constant motion 3. Particles do not interact (no attraction) 4. (KE) avg is directly proportional to temperature
- From this information under what conditions would real gases behave similarly to ideal gases? High temperature and low pressure are the conditions that allow a real gas to most closely approximate ideal gas behavior.
- What is the equation for Average Kinetic Energy? (KE) avg = 3 / 2 RT
- What does kinetic energy describe? The energy of motion.
- How does temperature effect kinetic energy? The higher the temperature the higher the kinetic energy.
- What is the equation for the root mean square velocity? μ rms = (3RT/M) 1/2
- How does mass affect the velocity? The greater the mass – the slower moving the particle.
- How does temperature affect the velocity? An increase in temperature results in an increase in velocity.
- If the plot represents the velocity distribution of 1.0 L of H 2 (g) versus 1.0 L of Ar (g) at STP, which plot corresponds to each gas? Plot A represents Ar (g) Plot B represents H 2 (g)
- If the plots correspond to the velocity distribution of 1.0 L of O 2 (g) at 273K and 1273K, which plot corresponds to each temperature? Plot A represents movement at 273K Plot B represents movement at 1273 K.
- Under which temperature condition would the O 2 (g) behave most ideally? The higher temperature – 1273 K.
- What is diffusion? Diffusion is the movement of a substance from higher concentration to lower concentration.
- What is effusion? Effusion is the passage of a gas through a tiny hole into an evacuated chamber.
- What is Graham’s Law? Compares the rate of effusion of 2 gases. Rate of effusion gas 1 = (M 2 ) 1/2 Rate of effusion gas 2 (M 1 ) 1/2
- It took 5.3 minutes for 1.0 L of helium to effuse through a porous barrier. How long will it take for 1.0L of chlorine gas to effuse under identical conditions? 22.2 minutes
- Increase in mass? Fewer collisions. No change to length of mean free path.
- Increase in diameter of particle? More collisions. Smaller mean free path.
- Increase concentration of gas? More collisions. Decreased mean free path.
- What is the Van Der Waal’s Equation? [P observed + a (n/V) 2 ] (V –nb) = nRT
- What is it correcting for? Pressure is corrected because particles do interact with each other. Volume corrected because the actual volume is smaller than ideal volume.
- What does the variable “a” have to do with? I always remember this variable by thinking “a” is for a ttraction. The greater the attraction between particles the greater the value of “a”.
- What does the variable “b” have to do with? I always remember this variable by thinking “b” is for b ig. The larger the particles the greater the value of “b”.
- Would He (g) or H 2 O (g) have a greater value of “a”? H 2 O
- Would He (g) or Xe (g) have a smaller value of “b”? He.
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Chemistry: The Kinetic Molecular Theory, homework help
User Generated
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A temperature increase will result in an increase in gas particle collisions with the walls of the container.
2 points Save Answer
Which of the following gases will diffuse most slowly at 35 degrees Celsius?
None of the above; they will all diffuse at the same rate.
3 points Save Answer
According to kinetic molecular theory, there are no forces of attraction between the particles of a liquid.
Of the three main states of matter, only gases can be compressed significantly.
Which of the following substances is a fluid?
In a car cylinder, a piston moves up and down inside a cylinder, causing the substance inside to expand and contract. Which type of substance could be inside the cylinder?
Liquid only
Liquid or solid only
Gas, liquid, or solid
The kinetic energy of carbon dioxide molecules in a can of soda is much higher when it is chilled than when it is at room temperature.
Which of the following would have the highest average kinetic energy?
Cl2 gas at 35 °C
F2 gas at 15 °C
O2 gas at 25 °C
N2 gas at 50 °C
The average kinetic energy for a volume of gas can be found by multiplying the following: 3/2, temperature (in Kelvin), and the gas constant, 0.0821 L*atm/mol K.
QUESTION 10
What is the average kinetic energy of 1 mole of a gas at 125 Kelvin? (R = 8.314 J/K-mol)
1.04 x 103 J
3.12 x 103 J
1.56 x 103 J
1.77 x 103 J
Explanation & Answer
Attached, you'll find the completed question sheet. I included an explanation where I thought it would be useful on the questions, but didn't include them for every problem due to time constraints. It's been a pleasure working with you, if there was anything else, feel free to reach out to me! :) QUESTION 1 A temperature increase will result in an increase in gas particle collisions with the walls of the container. TRUE – Temperature relates directly to the amount of energy in an object. This collision with the walls of the container are what creates pressure. Think of a sealed soda can—if you heat it up too much, the pressure inside will cause the can to burst!. FALSE QUESTION 2 Which of the following gases will diffuse most slowly at 35 degrees Celsius? O2 N2 𝑘 Cl2 – The formula for diffusion is: 𝑅𝑎𝑡𝑒 = (𝑎𝑡𝑜𝑚𝑖𝑐 𝑚𝑎𝑠𝑠)2 Where ‘k’ the const...
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Kinetic Molecular Theory Worksheet, Cheat Sheet for Chemistry
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