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(D) This process is known as free expansion.In free expansion,the gas expands into a vacuum,so the external pressure $P_{ext} = 0$.Therefore,the work

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Both $A$ and $B$ are correct.

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(D) This process is known as free expansion.In free expansion,the gas expands into a vacuum,so the external pressure $P_{ext} = 0$.Therefore,the work done $W = \int P_{ext} dV = 0$.According to the first law of thermodynamics,$\Delta Q = \Delta U + W$.Since the process is adiabatic,$\Delta Q = 0$.Substituting these values,we get $0 = \Delta U + 0$,which implies $\Delta U = 0$.For an ideal gas,internal energy $U$ is a function of temperature only $(U \propto T)$.Since $\Delta U = 0$,the change in temperature $\Delta T = 0$,meaning the temperature remains constant.Thus,both the heat supplied is zero and the temperature remains constant.

When a gas in a vacuum chamber expands suddenly,which of the following is true?

Similar Questions

Which of the following is $NOT$ a reversible process?

$A$ closed container is fully insulated from the outside. One half of it is filled with an ideal gas $X$ separated by a plate $P$ from the other half $Y$,which contains a vacuum as shown in the figure. When $P$ is removed,$X$ expands into $Y$. Which of the following statements is correct?

Which of the following is an irreversible process?

$Assertion :$ Reversible systems are difficult to find in the real world.
$Reason :$ Most processes are dissipative in nature.

There is no change in internal energy of an ideal gas when it undergoes

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