Most probable kinetic energy

The most probable speeds of methane and carbon dioxide are slower than the most probable speed of hydrogen, but CH4 and CO2 molecules have larger masses than H2. When kinetic energy calculations are repeated for these gases, they show that the most probable kinetic energy is the same for all three gases. 

Even though the speed distributions for these three gases peak at different values, the most probable kinetic energies are identical. 

C05-0117. Refer to Figure 5 to determine the following for O2 gas at 300 K (a) What is the most probable kinetic energy (b) What is the most probable speed ... 

In /z-space the most probable kinetic energy ep — mCp = kT, which differs from the average energy according to the equipartition principle,... 

What is the most probable kinetic energy of a proton in the interior of the sun (T= 1.5 x 107 K). What fraction of these protons has an energy greater than 0.5 MeV ... 

Surface- oxide Atom/Mo- lecule- Surface Configura- tion Ejected specie Threshold ev Most probable kinetic energy eV Desorption cross section cm REF. 

This graph shows a typical distribution of kinetic energies for a liquid at 25°C. The most probable kinetic energy lies at the peak of the curve. How would the curve look for the same liquid at 30°C ... 

Tritium is sometimes produced in fission. In reactors fueled with it is produced at the rate of 8.7 x 10 tritons per fission. The most probable kinetic energy of the tritons is about 7.5 MeV. 

In Fig. 2.4 ngln is plotted as a function of E for three different J s. For the line at 290 K we have marked the ergies kT and 3kT/2. While 3kT/2 (or rather 3RT/2) corresponds to the thermodynamic average translational energy, kT corresponds to the most probable kinetic energy the area under the curve is divided in two equal halves by the kT line. 

In Chapter 11 we encountered the term vapor pressure, referring to the temperature-dependent partial pressure of water [M< Section 11.5]. In fact, vapor pressure is another property of liquids that depends on the magnitude of intermolecular forces. The molecules in a liquid are in constant motion, and, like the molecules in a gas, they have a distribution of kinetic energies. The most probable kinetic energy for molecules in a sample of liquid increases with increasing temperature, as shown in Figure 12.9. If a molecule at the surface of a liquid has sufficient kinetic energy, it can escape from the liquid phase into the gas phase. This phenomenon is known as evaporation... 

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