# Kinetic molecular theory consider the following

• Test Prep
• 45
• 100% (4) 4 out of 4 people found this document helpful

This preview shows page 15 - 17 out of 45 pages.

15Kinetic Molecular Theory Consider the following statements about the kinetic theory of gases:A)The average kinetic energy of gas molecules is directly proportional to the absolute temperature.B)At constant temperature and pressure, all molecules of a gas in a sample will have exactly the same kinetic energy.C)One may deduce that at 0 K the most probable speed of ideal gas molecules is zero.D)At any constant temperature other than 0 K, the root mean square speed of a given mixture of ideal gas molecules is always higher than the average speed. E)The calculation of the average molecular speed of ideal gas molecules does not take into account the attractive forces between moleculesExplain if each statement is true or false.
Kinetic Molecular Theory An unidentified noble gas is knows to have a root mean square speed (urms) 2.0377 times smaller than the urmsof Ne at room temperature. Which noble gas is this?
Kinetic Molecular Theory Calculate the root-mean-square, average, and most probable speed in m/s at 25 degrees C for gaseous He atoms.
Kinetic Molecular Theory If 0.00354 mol N2(g) effuses through a tiny hole in 47 seconds, then how much H2(g) would effuse through the same orifice in 55 seconds?
Kinetic Molecular Theory How many of the following statements about the kinetic theory of gases are incorrect?i)The translational velocity of gas particle is inversely proportional to the absolutetemperature of the gasii)The collision of two gas molecules is assumed to be elasticiii)Boyle’s Law can be proven using the kinetic theory of gasesiv)According to the Maxwell-Boltzmann distribution of gas velocities, the root meansquare speed is greater than the average speed.v)The absolute temperature of a gas is proportional to the kinetic energy of a gas.
16vi)The root-mean-square speed at 25 °C for gaseous Ar atoms is 432 m/s.
Kinetic Molecular Theory Consider the following statements about the kinetic theory of gases:i.The average kinetic energy of gas molecules is directly proportional to the absolute temperatureii.At constant temperature and pressure, all molecules of a gas in a sample will have exactly the same kinetic energyiii.One may deduce that at 0K the most probable speed of ideal gas molecules is zeroiv.At any constant temperature other than 0K, the root mean square speed of a given mixture of ideal gas molecules is always higher than the average speedv.The calculation of the average molecular speed of ideal gas molecules does not take into account the attractive forces between moleculesHow many of the above statements are incorrect?