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Formula from Chapter 9: chemical amount of a pure gas (ideal gas law)

You can use this if: the sample is a gas (and the pressure is low and the temperature high)

\(R\) \(= 8.314\ \frac{\mathrm{J}}{\mathrm{mol}\ \mathrm{K}}\)


\(n\) \(= 0.53\ \mathrm{mol}\)


\(T\) \(= 298.15\ \mathrm{K}\)


\(P\) \(= 1.00\ \mathrm{atm}\)


\(V_{\mathrm{gas}}\) \(= \dfrac{n \cdot R \cdot T}{P}\)

\(\ \ \ =\dfrac{0.53\ \mathrm{mol} \cdot 8.314\ \frac{\mathrm{J}}{\mathrm{mol}\ \mathrm{K}} \cdot 298.15\ \mathrm{K}}{1.00\ \mathrm{atm}}\)

\(\ \ \ =\dfrac{4.406\ \frac{\mathrm{J}}{\mathrm{K}} \cdot 298.15\ \mathrm{K}}{1.00\ \mathrm{atm}}\)

\(\ \ \ =\dfrac{1314.\ \mathrm{J}}{1.00\ \mathrm{atm}}\)

\(\ \ \ =0.0130\ \mathrm{m}^{3}\)