To prove this, we will have to use 3 equations, 2 of them related to ideal gases:
(i) pV = nRT
(ii) p = 1/3 d <c2>
(iii) Ek = 1/2 mv2
First of all, an ideal gas has no intermolecular forces. Thus, its molecules have no potential energy.
The internal energy of any system can be defined as the sum of the randomly distributed microscopic potential energy and kinetic energy of the molecules of the system.
It is thus evidently clear that the internal energy of an ideal gas is entirely kinetic. (Ep being zero)
So, U = 1/2 m <c2> (for an ideal gas)
From (i) and (ii), <c2> = 3p/d = 3pV/m = 3nRT/m (d= m/V)
Substituting in the appropriate equation, we get:
U = 1/2 m (3nRT/m)
U = 3/2 nRT
From the above equation, it can be concluded that for a fixed mass of an ideal gas, internal energy is proportional to the thermodynamic temperature. (fixed mass such that n is constant)
The one and only macroscopic thermodynamic property that the internal energy of an ideal gas depends on is its temperature.
Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.
it increases
Yes, temperature and kinetic energy are always equal except when going through a phase change, during which temperature stays the same, potential energy increases, and bonds are made/broken. In the case of gas, kinetic energy is equal to temperature unless condensing or depositing.
If the volume remains constant, the pressure will increase as the temperature increases. In an ideal gas (under normal conditions, gases have a behavior that's close to that of an ideal gas), the pressure is directly proportional to the temperature. Assuming, of course, that the temperature is measured in Kelvin.
The internal energy of the ideal gas is a function of temperature alone. This isJoule's Law.
The one and only macroscopic thermodynamic property that the internal energy of an ideal gas depends on is its temperature.
Temperature. PV = nRT. Both sides of this equation have dimensions of energy.n = number of moles; R is the Ideal Gas Constant; and T is absolute Temperature. So for a given amount of gas, the energy is directly proportional to Temperature.
Lots of things are true... Here are some:* For constant pressure, the volume of an ideal gas is directly proportional to the absolute temperature. * For constant volume, the pressure of an ideal gas is directly proportional to the absolute temperature.
What is the ideal set temperature for washing machines to conserve energy?
Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.Other things being equal, it is directly proportional to the temperature. It is also directly proportional to the amount of gas.
There is no such law. The Ideal Gas Law states that pressure is proportional to the number of molecules Pressure x Volume = number x Ideal gas constant x Temperature
it increases
directly proportional to the Kelvin temperature
Yes, temperature and kinetic energy are always equal except when going through a phase change, during which temperature stays the same, potential energy increases, and bonds are made/broken. In the case of gas, kinetic energy is equal to temperature unless condensing or depositing.
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The ideal internal temperature for poultry is 160 degrees held for at least 30 seconds.