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Chemistry
OpenStudy (anonymous):

For this question, use the main assumptions of the Kinetic Molecular Theory of gases: 1. Gases are made up of molecules which are relatively far apart. 2. The molecules are in motion at high speeds. 3. The molecular collisions are perfectly elastic. 4. Increase in temperature increases the kinetic energy of the molecules. Which of the assumptions explains the pressure which a gas exerts? 1 2 3 4 1 and 2 2 and 4 For this question, use the main assumptions of the Kinetic Molecular Theory of gases: 1. Gases are made up of molecules which are relatively far apart. 2. The molecules are in motion at high speeds. 3. The molecular collisions are perfectly elastic. 4. Increase in temperature increases the kinetic energy of the molecules. Which of the assumptions explains the pressure which a gas exerts? 1 2 3 4 1 and 2 2 and 4 @Chemistry

7 years ago
OpenStudy (anonymous):

For this question, use the main assumptions of the Kinetic Molecular Theory of gases: 1. Gases are made up of molecules which are relatively far apart. 2. The molecules are in motion at high speeds. 3. The molecular collisions are perfectly elastic. 4. Increase in temperature increases the kinetic energy of the molecules. Which of the above assumptions accounts for the compressibility of gases as compared to liquids and solids? 1 2 3 4 2 and 3 3 and 4

7 years ago
OpenStudy (anonymous):

For this question, use the main assumptions of the Kinetic Molecular Theory of gases: 1. Gases are made up of molecules which are relatively far apart. 2. The molecules are in motion at high speeds. 3. The molecular collisions are perfectly elastic. 4. Increase in temperature increases the kinetic energy of the molecules. The idea that no energy is lost when gas molecules hit the walls of a container or each other is explained by 1 2 3 4

7 years ago
OpenStudy (anonymous):

When the pressure of a gas doubles, the volume: doubles triples halves quarters remains constant

7 years ago
OpenStudy (anonymous):

there s no answer....

6 years ago
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