How would the graph in Figure 9.12 change if the number of moles of gas in the sample used to determine the curve were doubled?

A mole is used to describe an amount that cannot be quantified in grams or milligrams. So, a mole is a unit of measurement for a number of atoms, ions, or molecules.

Charles' law is depicted in a different way in this diagram.

Statement of Charles’ law:

Given a certain quantity of gas and a fixed pressure, the ratio between temperature in kelvin and volume is constant.

\begin{aligned} {\frac{V}{T}}=\texttt{constant}\end{aligned}

Figure 9.12 shows a graph

The graph depicts the volume versus the temperature of 1 mole of gas at 1 bar of pressure as an example of Charles’ law.

In accordance with Charles’ law in a rearranged form, V = const×T, const being the slope of the line on the graph. The resultant curve is linear (y = ax, a is slope).

However, we know that Charles’ law is a special cascade of the ideal gas law.

pV =nRT

T refers to the temperature in kelvin degrees, and V stands for volume.

Furthermore, n represents the number of moles, p represents the pressure of the same material, and R represents the universal ideal gas constant.

The ideal gas law states that

pV = nRT

\begin{aligned}V=\frac{nR}{p}\times T\end{aligned}

\begin{aligned}const= \frac{nR}{p}\end{aligned}

\begin{aligned}const= \frac{nR}{p}\end{aligned} is the slope of the line on the graph in Figure 9.12

therefore, if n doubles, the slope doubles, making the line twice as steep.