Kinetie Molecular Theory To explain the behavior of gases, the following theory

Question

Kinetie Molecular Theory To explain the behavior of gases, the following theory for the "ideal" gas has been A. Gases are comprised of very small particles whose diameters are very small compared with the distances between particles (Gas volumes are mostly empty space). 3. These particles are moving at very high speeds. O2 molecules move about 1000 miles/hr @ 25°C, and Hz molecules move about 4 times that rate C. Particles collide with themselves and the walls of the container in perfectly elastic collisions with no change to the total energy of motion of the particles (energy can be transferred from one particle to another but the total energy of the system remains constant). Gas pressure is caused by the gas particles hitting the sides of the container. Both the frequency and the force of these collisions affect gas pressure. D. There are no attractive forces between gas particles. 20. Explain to your teammates Boyle's Law in terms of KM theory: why is the pressure of a gas inversely proportional to its volume? 21. Explain, using KM Theory, the relationship between the temperature of a gas and the pressure of the gas. How about temperature and volume? proportional to the number of moles of the gas? Why doesn't one mole of an element like xenon occupy more space than one mole of helium atoms, which is a much smaller atom? 22. How does KM theory account for Avogadro's Law: the volume of a gas is 281

Explanation / Answer

20.

Because ther is a large distance between particles and hence on increasing pressure the molecules will come closer and occupy lesser volume.

So, P is inversely propotional to V

21.

As the temperature increases the kinetic energy of the molecules will aslo increase and hence hte moving velocity of molecules increase. So, they colloide the walls of the container more frequently and hence exerts more pressure.

So, P directly proportional to T

Similary on creasing temperature the gas molecules tries to move far apart from one another as they aquire more kinetic energy and hence occupy higher volume.

SO, V is directly proportional to T

22.

Here it is assumed that there exists no interactions among gas molecules. And hence the at given temperature and pressure, equal volumes of gases have equal number of moles without considering the nature of gases.

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