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NCERT Class XI Chemistry States of Matter Solutions

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Question : 7 of 23
Marks: +1, -0
What will be the pressure exerted by a mixture of 3.2 g of methane and 4.4 g of carbon dioxide contained in a 9 dm3\mathrm{dm}^3 flask at 27°C?
Solution:  
nCH4n_{\mathrm{CH}_4} = 3.216\frac{3.2}{16} = 0.2 mole ; nCO2n_{\mathrm{CO}_2} = 4.444\frac{4.4}{44} = 0.1 mole
PCH4P_{\mathrm{CH}_4} = nCH4VRT\frac{n_{\mathrm{CH}_4}}{V} RT = 0.2VRT\frac{0.2}{V} RT ; PCO2P_{\mathrm{CO}_2} = 0.1VRT\frac{0.1}{V} RT
PmixtureP_{\text{mixture}} = PCH4+PCO2P_{\mathrm{CH}_4}+P_{\mathrm{CO}_2} = 0.2 × RTV\frac{RT}{V} + 0.1 × RTV\frac{RT}{V} = 0.3×0.0821×3009\frac{0.3 \times 0.0821 \times 300}{9} = 0.821 atm
= 0.821 × 101325 = 8.318 × 10410^4 Pa [Since 1 atm = 101325 Pa]
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