0.2 g of a gas X occupies a volume of 0.44 L at the same pressure and temperature. Under identical conditions of P and T, 0.1 g of CO2 gas occupies 0.32 L. Gas X can be :
Correct answer: B. SO2
- A. O2
- B. SO2
- C. NO
- D. C4H10
Explanation
To determine the identity of gas X, we compare the given conditions for CO2 and gas X under the same pressure and temperature. Using the formula:PV = nRT, where n is the number of moles, we can determine the molar mass of gas X.For CO2, 0.1 g occupies 0.32 L. The molar mass of CO2 is 44 g/mol.For gas X, 0.2 g occupies 0.44 L. Using the volume ratios, we find the molar mass of gas X to be approximately 64 g/mol.Therefore, gas X is most likely SO2, which matches the calculated molar mass. Options like O2 and NO have significantly lower molar masses, and C4H10 does not align with the calculated molar mass, confirming that SO2 is the correct answer.
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About Gases
Gas behaviour is explained through the kinetic molecular theory and the relationships among pressure, volume and temperature. Work includes STP, Boyle's and Charles's laws, absolute zero, the ideal gas equation, and the distinction between ideal and real gases, especially the effects of intermolecular forces and molecular volume.
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