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Why internal energy of an ideal gas depends only on temperature?

Why internal energy of an ideal gas depends only on temperature?

Pressure and volume change while the temperature remains constant. Since no work or heat are exchanged with the surrounding, the internal energy will not change during this process. Thus, the internal energy of an ideal gas is only a function of its temperature.

What is the relation of internal energy of an ideal gas with gas temperature?

The internal energy of an ideal gas is therefore directly proportional to the temperature of the gas. In this equation, R is the ideal gas constant in joules per mole kelvin (J/mol-K) and T is the temperature in kelvin. The internal energy of systems that are more complex than an ideal gas can’t be measured directly.

What happens when an ideal gas is compressed?

During compression, the volume (V) of a gas decreases. When this happens, the pressure (P) of the gas increases if the number of moles (n) of gas remains constant. If you keep the pressure constant, reducing the temperature (T) also causes the gas to compress.

What is isothermal expansion of an ideal gas?

Isothermal Expansion This shows the expansion of gas at constant temperature against weight of an object’s mass (m) on the piston. Temperature is held constant, therefore the change in energy is zero (U=0). So, the heat absorbed by the gas equals the work done by the ideal gas on its surroundings.

When an ideal gas is compressed adiabatically its temperature?

Solution : When an ideal gas is compressed adiabatically, its temperature riese, because heat produced cannot be lost to the surroundings. Each molecules has more KE than before because of collisions of molecules with moving parts of the wall (i.e. Piston compressing the gas).

When an ideal gas is compressed adiabatically and reversibly The final temperature is?

When an ideal gas is compressed adiabatically and reversibly, the final temperature is higher than initial temperature. As dU is positive , then temperature must be increased . So, When an ideal gas is compressed adiabatically and reversibly, the final temperature is higher than initial temperature.

What is the ratio of final volume to initial volume if the gas is compressed adiabatically till its temperature is doubled?

The ratio of its final volume to initial volume will be. ⇒V

What is the ratio of slopes of PV graphs of adiabatic and isothermal process?

The slope of P-V graph is dP/dVFor an isothermal process PV = constantSo dP/dV = P/V → 1For an adiabatic process PVY = constant dP/dV = YP/V → 2Divide 2 by 1 So the ratio of adiabatic slope to isothermal slope is Y.

What is free expansion of ideal gas?

The Joule expansion (also called free expansion) is an irreversible process in thermodynamics in which a volume of gas is kept in one side of a thermally isolated container (via a small partition), with the other side of the container being evacuated.

What is the work done for an ideal gas isothermal process?

For an ideal gas, from the ideal gas law PV = NkT, PV remains constant through an isothermal process. A curve in a P-V diagram generated by the equation PV = const is called an isotherm. For an isothermal, reversible process, the work done by the gas is equal to the area under the relevant pressure -volume isotherm.