The following graph represents the T-V curves of an ideal gas (where T is the temperature and V the volume) at three pressures P₁, P₂ and P₃ compared with those of Charles’s law represented as dotted lines.

Then the correct relation is:

The correct relation is: P₁ > P₂ > P₃

To understand the relationship between the pressures P₁, P₂, and P₃ from the temperature-volume (T-V) graph, we can use the ideal gas law:
$PV=nRT$
where:
• P is the pressure of the gas,
• V is the volume of the gas,
• n is the number of moles of the gas,
• R is the universal gas constant, and
• T is the absolute temperature.

We can rearrange this equation to express temperature (T) as a function of volume (V):
$T=\left(\frac{P}{nR}\right)V$

In a T-V graph where temperature (T) is plotted on the vertical y-axis and volume (V) is plotted on the horizontal x-axis, the slope of the curve represents:
$\text{Slope}=\frac{T}{V}=\frac{P}{nR}$

Since the number of moles (n) and the gas constant (R) are constant, the slope of each line is directly proportional to the pressure (P) of the gas:
$\text{Slope}\propto P$

Alternatively, if we draw a vertical line representing a constant volume (V = constant) across the curves, the pressure becomes directly proportional to the temperature:
$P\propto T$
From the graph, at any given constant volume, the temperature corresponding to the curve for P₁ is the highest, followed by P₂, and then P₃ (T₁ > T₂ > T₃).
Therefore, the corresponding pressures follow the same order: P₁ > P₂ > P₃.