Question

The P-V diagram of path followed by one mole of perfect gas in a cylindrical container is shown in figure, the work done when the gas is taken from state A to state B is:
                                 

$\begin{align}
  & (A)2{{P}_{2}}{{V}_{1}}\left[ 1-\sqrt{\dfrac{{{V}_{2}}}{{{V}_{1}}}} \right] \\
 & (B)2{{P}_{1}}{{V}_{1}}\left[ 1-\sqrt{\dfrac{{{V}_{1}}}{{{V}_{2}}}} \right] \\
 & (C)2{{P}_{2}}{{V}_{2}}\left[ 1-\sqrt{\dfrac{{{V}_{1}}}{{{V}_{2}}}} \right] \\
 & (D)2{{P}_{1}}{{V}_{2}}\left[ 1-\sqrt{\dfrac{{{V}_{1}}}{{{V}_{2}}}} \right] \\
\end{align}$

Answer 1

Hint: We have been given the condition that, $P{{V}^{\dfrac{1}{2}}}=k$ ,where k is any arbitrary constant. Now, this is an example of a polytropic process. So we will use the formula of work done in taking a gas from initial state to a final state of a polytropic process.

Complete answer:
It has been given in the question:
The initial parameters of gas are denoted by the following terms:
Initial volume : ${{V}_{1}}$
Initial pressure: ${{P}_{1}}$
Initial temperature: ${{T}_{1}}$
And, the final parameters of the gas are given by the following terms:
Final volume : ${{V}_{2}}$
Final pressure : ${{P}_{2}}$
Final temperature: ${{T}_{2}}$
Now, once we have defined the initial and final parameters of the gas, we can proceed ahead with calculating the work done in the given process.
As it is given:
$\Rightarrow P{{V}^{\dfrac{1}{2}}}=k$
This is a Polytropic process, with the value of :
$\Rightarrow n=\dfrac{1}{2}$
Now, the formula for work done in a polytropic process is given by the following equation:
$\Rightarrow W=\dfrac{{{P}_{1}}{{V}_{1}}-{{P}_{2}}{{V}_{2}}}{n-1}$
Putting the value of (n) in the above equation, we get:
 $\begin{align}
  & \Rightarrow W=\dfrac{{{P}_{1}}{{V}_{1}}-{{P}_{2}}{{V}_{2}}}{\dfrac{1}{2}-1} \\
 & \Rightarrow W=2\left( {{P}_{2}}{{V}_{2}}-{{P}_{1}}{{V}_{1}} \right) \\
\end{align}$
Taking ${{P}_{2}}{{V}_{2}}$common out of the bracket in the right-hand side of the equation, we get the work done as:
 $\Rightarrow W=2{{P}_{2}}{{V}_{2}}\left( 1-\dfrac{{{P}_{1}}{{V}_{1}}}{{{P}_{2}}{{V}_{2}}} \right)$ [Let this expression be equation number (1)]
Now, using the given polytropic function, we can write:
$\begin{align}
  & \Rightarrow {{P}_{1}}{{({{V}_{1}})}^{\dfrac{1}{2}}}=k \\
 & \Rightarrow {{P}_{1}}{{({{V}_{1}})}^{\dfrac{1}{2}}}\times {{(V)}^{\dfrac{1}{2}}}=k{{(V)}^{\dfrac{1}{2}}} \\
 & \Rightarrow {{P}_{1}}{{V}_{1}}=k{{({{V}_{1}})}^{\dfrac{1}{2}}} \\
\end{align}$
Similarly, for the final state of gas we can write:
$\Rightarrow {{P}_{2}}{{V}_{2}}=k{{({{V}_{2}})}^{\dfrac{1}{2}}}$
Using these two equations in equation number (1), we get:
$\begin{align}
  & \Rightarrow W=2{{P}_{2}}{{V}_{2}}\left( 1-\dfrac{k\sqrt{{{V}_{1}}}}{k\sqrt{{{V}_{2}}}} \right) \\
 & \therefore W=2{{P}_{2}}{{V}_{2}}\left( 1-\dfrac{\sqrt{{{V}_{1}}}}{\sqrt{{{V}_{2}}}} \right) \\
\end{align}$
Hence, the work done in taking gas from $1\to 2$ under the given polytropic process is $2{{P}_{2}}{{V}_{2}}\left( 1-\sqrt{\dfrac{{{V}_{1}}}{{{V}_{2}}}} \right)$ .


So, the correct answer is “Option C”.

Note: In a polytropic process, (n) can take any value. If we keep on varying (n) we will see that for different values of (n), we get different processes. For example: for, $n=0$ , the process will become isobaric. For, $n=1$, the process will become isothermal, etc. Thus all the basic processes are a subset of the polytropic process.