3.0 g of a gas occupies the same volume as 1.0 g of methane gas, CH4, at the same temperature and pressure. The gas could be: [ Molar Masses (g mol-1) C = 12.0 H = 1.00 O = 16.0 N =14.0 ]

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To compare the gases at the same temperature and pressure, use the fact that equal volumes contain equal numbers of moles for ideal gases. First, determine the number of moles in 1.0 g of CH4: moles = mass / molar mass = 1.0 g / 16.0 g/mol = 0.0625 mol. Since 3.0 g of the unknown gas occupies the same volume as 1.0 g CH4, it must contain the same number of moles, i.e., 0.0625 mol. Now compute the molar mass of the unknown gas: molar mass = mass / moles = 3.0 g / 0.0625 mol = 48.0 g/mol.

Option a: CO2 has a molar mass of about 44 g/mol, which does not match the calculated 48 g/mol, so this is not correct.
Option b: NO2 has a molar mass of about 46 g/mol, also not equal to 48 g/mol, so this is not correct.
Option c: O2 has a molar mass of 32 g/mol, far from 48 g/mol, so this is not correct.
Option d: O3 (ozone) has a molar mass of 3 × 16 = 48 g/mol, which exactly matches the calculated value, making this the correct choice.

MUF0041 Chemistry Unit 1 - Semester 1, 2025 Area of Study 3 Test 1(Gases/Solids/Liquids)

3.0 g of a gas occupies the same volume as 1.0 g of methane gas, CH4, at the same temperature and pressure. The gas could be: [ Molar Masses (g mol-1) C = 12.0 H = 1.00 O = 16.0 N =14.0 ]

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