The moles of helium gas occupied a volume of 10 l at 2 7 ∘ C . The gas is first expanded at constant pressure until the volume is doubled. It then undergoes adiabatic change until the temperature retu

Question

The moles of helium gas occupied a volume of 10 l at 2 7 ∘ C . The gas is first expanded at constant pressure until the volume is doubled. It then undergoes adiabatic change until the temperature returns to its initial value. Which diagram is correct for this process?

TestHub · Accepted Answer

Since the gas is first expanded at a constant pressure, we observe the graph shown below:

In this plot,

$\frac{V _{X}}{T _{X}} = \frac{V _{A}}{T _{A}}$

$\frac{10}{300} = \frac{20}{T _{A}}$

$T_{A} = 600 K$ .

In the adiabatic process, since the temperature returns to its initial value of 300 K, this indicates that a decrease in temperature occurred, which signifies an expansion in the volume of the container has occurred.

Therefore, (c) is the correct option.

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