it increases
The one and only macroscopic thermodynamic property that the internal energy of an ideal gas depends on is its temperature.
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)
In a container of constant volume, when the gas is heated, thermal energy is converted to kinetic energy. This increase in kinetic energy causes the gas particles to accelerate. This acceleration of particles causes the particles to crash into each other, increasing pressure. Because it is a closed container, the number of particles and the volume the particles take up remain the same.
The first law of thermodynamics states that: DU = DQ + DW where DU is the increase in the internal energy of the gas DQ is the heat supplied to the system and DW is the work done ON the system For an adiabatic process, DQ = 0 Therefore, DU = DW It can be thus easily seen that for the internal to increase (DU +ve), DW must be positive, that is work has to be done on the system (in this case the ideal gas). Hence, the gas should be compressed.
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The one and only macroscopic thermodynamic property that the internal energy of an ideal gas depends on is its temperature.
The internal energy of the ideal gas is a function of temperature alone. This isJoule's Law.
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)
ideal ammeter has zero internal resistance
internal resistance is always infinite in ideal current source .the internal resistance is in shunt with current source
zero
In a container of constant volume, when the gas is heated, thermal energy is converted to kinetic energy. This increase in kinetic energy causes the gas particles to accelerate. This acceleration of particles causes the particles to crash into each other, increasing pressure. Because it is a closed container, the number of particles and the volume the particles take up remain the same.
The first law of thermodynamics states that: DU = DQ + DW where DU is the increase in the internal energy of the gas DQ is the heat supplied to the system and DW is the work done ON the system For an adiabatic process, DQ = 0 Therefore, DU = DW It can be thus easily seen that for the internal to increase (DU +ve), DW must be positive, that is work has to be done on the system (in this case the ideal gas). Hence, the gas should be compressed.
What is the ideal set temperature for washing machines to conserve energy?
yes
Under ideal conditions, population increases.
Zero out impedance and infinite internal resistance. - Divya Naveenan