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Calculate the volume occupied by \(8.8 \mathrm{~g}\) of \(\mathrm{CO}_2\) at 31. \(1^{\circ} \mathrm{C}\) and 1 bar pressure. \(R=0.083\) bar \(^2 \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\).
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\(\mathrm{PV}=\mathrm{nRT}\) or, \(\mathrm{V}=\frac{\mathrm{nRT}}{\mathrm{P}}=\frac{\mathrm{wRT}}{\mathrm{MP}}\left(\right.\) because \(\left.\mathrm{n}=\frac{\mathrm{w}}{\mathrm{M}}\right)\)
\(\mathrm{V}=\frac{8.8 \mathrm{~g}}{44 \mathrm{~g} \mathrm{~mol}^{-1}} \times \frac{0.083 \mathrm{bar} \mathrm{L} \mathrm{K}^{-1} \mathrm{~mol}^{-1} \times(273+31.1) \mathrm{K}}{1 \mathrm{bar}}\)
\(=5.05 \mathrm{~L} \text {. }\)
\(\mathrm{V}=\frac{8.8 \mathrm{~g}}{44 \mathrm{~g} \mathrm{~mol}^{-1}} \times \frac{0.083 \mathrm{bar} \mathrm{L} \mathrm{K}^{-1} \mathrm{~mol}^{-1} \times(273+31.1) \mathrm{K}}{1 \mathrm{bar}}\)
\(=5.05 \mathrm{~L} \text {. }\)
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