How would the graph in Figure \({\rm{9}}{\rm{.13}}\) change if the number of moles of gas in the sample used to determine the curve were doubled?

A mole is used to describe amounts that cannot be quantified in gramsor milligrams. As a result, a mole is a unit of measurement for a number of atoms, ions, or molecules.

If the temperature and numberof gas molecules remain constant, Boyle's law asserts that the pressure and volume of the gas are inversely proportional. This can be written as

\({{\rm{p}}_{\rm{1}}}{{\rm{V}}_{\rm{1}}}{\rm{ = }}{{\rm{p}}_{\rm{2}}}{{\rm{V}}_{\rm{2}}}\).

The beauty of this connection (Avogadro's law) is that if we double the number of molecules, our initial volume will be greater.

\({\rm{n = }}\frac{{\rm{V}}}{{{{\rm{V}}_{\rm{m}}}}}\).

Here,\({{\rm{V}}_{\rm{m}}}\)is the molar volume determined at a given pressure and temperature. This means that we will have a larger beginning volume, but according to Boyle's rule, the change in volume is still inversely proportional to the change in pressure.

Therefore, the curve would have the same shape as before, but it would be relocated to the right and higher up.