Use the kinetic-molecular theory to explain the following: Why the pressure of a
ID: 954872 • Letter: U
Question
Use the kinetic-molecular theory to explain the following: Why the pressure of a gas doubles if its volume is reduced to half at constant temperature? Why the pressure of a gas is increased if the gas is heated in a closed, rigid container? Why oxygen can be added to a rigid container which is filled with nitrogen? Why a helium filled rubber balloon will collapse quicker than if it was filled with nitrogen? Why some gases will liquefy more readily than others? Why gases deviate from the gas laws at low temperature and high pressure? Explain why the volumes of real gases actually do not become zero at absolute zero. Which gas will diffuse faster, H_2 or He? Show, by way of a calculation, how many times faster.Explanation / Answer
ANSWER
Dear candidate you have asked three different questions with first question having six parts. As per chegg guidelines one question one time and that too should not have more than four parts. Here we solve first question with all parts.
1. (a) According to kinetic molecular theory pressure of a gas is the result of bombardment of gas particles with the walls of the container. Hence more the number of particles per unit volume striking the walls of container more will be the pressure. When volue is decreased the number of molecules per unit voume (density) increases hence the pressure increases
(b) The kinetic energy of gas molecules increases with increase in temperature. As a result the number of collisions of a gas molecule per unit time increase, this results in increase in pressure
(c) There exist large spaces between the gs molecules. Hence a gas can acommodate the other gas when mixed in rigid container
(d) The gas molecules have a finite size. The size of He molecule is smaller than that of N2 and can escape through the pores f balloon. That is why H filles balloones collapse quicker.
(e) There exists a force of attraction between the molecules of gas. This attractive force is different in different gases. The which has a stronger force of attraction between its molecules will liquify easily.
(f) Ideal gas molecules do not have a force of attraction between then and these molecules are moving with very high speeds. At low temperature and high pressure the speed of gas molecules is less and the force of attraction is high. That is the reason why gases deviate from ideal behaviuor at low temperature and high pressure.
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