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NCERT Class XI Chemistry States of Matter Solutions

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Question : 17 of 23
Marks: +1, -0
Calculate the volume occupied by 8.8 g of CO2\mathrm{CO}_2 at 31.1°C and 1 bar pressure. (R = 0.083 bar L K−1 mol−1\mathrm{L\,K^{-1}\,mol^{-1}})
Solution:  
According to ideal gas equation, PV = nRT
n = 8.844\frac{8.8}{44} moles , P = 1 bar , T = 273 + 31.1 = 304.1 K ,
V = ?
R = 0.083 bar LK−1mol−1\mathrm{LK^{-1}mol^{-1}}
Now , V = nRTP\frac{nRT}{P} =
(8.844 moles)×(0.083 bar LK−1mol−1)×(304.1 K)1 bar\frac{ \left( \frac{8.8}{44} \,\text{moles} \right) \times \left( 0.083 \,\mathrm{bar}\,\mathrm{LK^{-1}mol^{-1}} \right) \times \left( 304.1 \,\mathrm{K} \right) }{ 1 \,\mathrm{bar} }
= 5.05 L
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