internal energy ideal gas
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Re: internal energy ideal gas
For an isothermal expansion of an ideal gas, the amount of work that the system does is replaced by the same amount of heat (which is how the system is isothermal). Since we know that ∆U=q+w, the work done to the system is going to be negative (for expansion) and the heat would be put into the system (the same value but positive), so overall ∆U would equal 0.
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Re: internal energy ideal gas
In Isothermal process the temperature is constant. The internal energy is a state function dependent on temperature. Therefore, the internal energy change is 0.
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Re: internal energy ideal gas
The work done is replaced by heat so Q = -W. Since delta U = Q + W, it would be 0.
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Re: internal energy ideal gas
∆U = 0 for an isothermal expansion of an ideal gas because the work that is done within the system is replaced by energy in the form of heat. This means that Q = -W, which also can be written as ∆U = Q + W, which also equals 0.
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