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BioPhysicist
BioPhysicist
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In adiabatic expansion, does the internal energy of an ideal gas decreasesdecrease?

By First Law of thermodynamic, for an ideal gas, if there isn’t heat transfer, work done by the gas is equal to decrease in internal energy of the gas.

Suppose that I have a perfectly-insulated syringe closed at one end and a frictionless piston on the other. The syringe initially contain ideal gas of volume V$V$. If I pulled the piston outward, the volume of gas would increase. Since I am the one applying force, work is done by me instead of by the contained gas. So, in this case, does the internal energy of gas remain constant?

In adiabatic expansion, internal energy of gas decreases?

By First Law of thermodynamic, for an ideal gas, if there isn’t heat transfer, work done by the gas is equal to decrease in internal energy of the gas.

Suppose that I have a perfectly-insulated syringe closed at one end and a frictionless piston on the other. The syringe initially contain ideal gas of volume V. If I pulled the piston outward, the volume of gas increase. Since I am the one applying force, work is done by me instead of by the contained gas. So, in this case, does the internal energy of gas remain constant?

In adiabatic expansion does the internal energy of an ideal gas decrease?

By First Law of thermodynamic, for an ideal gas, if there isn’t heat transfer, work done by the gas is equal to decrease in internal energy of the gas.

Suppose that I have a perfectly-insulated syringe closed at one end and a frictionless piston on the other. The syringe initially contain ideal gas of volume $V$. If I pulled the piston outward, the volume of gas would increase. Since I am the one applying force, work is done by me instead of by the contained gas. So, in this case, does the internal energy of gas remain constant?

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JF9199
JF9199
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In adiabatic expansion, internal energy of gas decreases?

By First Law of thermodynamic, for an ideal gas, if there isn’t heat transfer, work done by the gas is equal to decrease in internal energy of the gas.

Suppose that I have a perfectly-insulated syringe closed at one end and a frictionless piston on the other. The syringe initially contain ideal gas of volume V. If I pulled the piston outward, the volume of gas increase. Since I am the one applying force, work is done by me instead of by the contained gas. So, in this case, does the internal energy of gas remain constant?