How is the pressure versus volume graph for a sample of an ideal gas at constant temperature?

Hint:. The following question is based on ideal gas equation i.e. PV= nRT. Here V is volume of gas in liters (L), P is pressure in atmospheres (atm), T is temperature if gas in kelvins (K) and n is moles of gas taken (mol).

Complete step by step answer:
The question about a condition of gas where temperature is kept constant and pressure change is studied with change in volume or vice versa. To obtain the answer we will consider that the gas is an ideal one. An ideal gas is defined as a hypothetical gaseous substance whose behavior is independent of attractive and repulsive forces and can be completely described by the ideal gas law. The ideal gas law equation is PV=nRT.
Where V= Volume of gas in liters (L)
P = Pressure in atmospheres (atm)
T = Temperature if gas in kelvins (K)
n = Moles of gas taken (mol)
R = Universal gas constant.

Now R is a constant, n is also constant as the number of moles are not changing during the process and T is constant too, as said in the question. So the ideal gas equation now become:
PV= Constant
$P \propto \dfrac{1}{V}$
This is Boyle’s law too and the graph obtained from this relation is rectangular hyperbola.

Note: Don’t get confused with the indirectly proportional relation of P and V, as indirectly proportional variables provide straight line graphs with negative slope. Here the graph depends on the constant temperature to which it makes its rectangular hyperbola.