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## Standard molar volume

- For one mole of an ideal gas:
- $V=\frac{\mathrm{R.}T}{p}\text{with n = 1}$

For all ideal gases, one mole of gas takes up a volume of 22.4141 $\text{L.}$ on when the pressure is 1.013 $\text{bar}$ = 1 $\text{atm}$ and the temperature 0 $\text{\xb0 C}$ amounts to. This volume is called the standard molar volume.

Unfortunately the temperature corresponds to 0 $\text{\xb0 C}$ not the standard thermodynamic temperature of 25 $\text{\xb0 C}$. The molar volume of the latter is 24.47 $\text{L.}$.

From the general gas equation, a conversion formula for changed conditions can be set up for a certain amount of gas under known conditions. the end

- Condition 1
- $${p}_{1}\cdot {V}_{1}\text{}=n\cdot \mathrm{R.}\cdot {T}_{1}$$
- Condition 2
- $${p}_{2}\cdot {V}_{2}\text{}=n\cdot \mathrm{R.}\cdot {T}_{2}$$
- is obtained by eliminating $n\cdot \mathrm{R.}$
- $$\frac{{\text{p}}_{\text{1}}\cdot {\text{V}}_{\text{1}}}{{\text{T}}_{\text{1}}}=\frac{{\text{p}}_{\text{2}}\cdot {\text{V}}_{\text{2}}}{{\text{T}}_{\text{2}}}$$