A gas sample exhibits a density of 0.0847 g/L at 17°C and 760 torr pressure. Identify the gas.
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Answer: B. He
Explanation
Calculating the molar mass using the ideal gas density equation yields roughly four grams per mole. This calculated molecular weight corresponds directly to the atomic mass of helium gas. Low gas density under given ambient conditions confirms the presence of a very light elemental gas. The ideal gas law relates pressure, volume, temperature, and moles for simple gas systems. Density is defined as mass divided by volume, which can be rearranged to find molar mass. Helium is a noble gas known for being chemically inert and extremely light compared to air.
Analytical chemists use density measurements to identify unknown gas samples in laboratory settings. Helium is widely used in cryogenics, leak detection, and inflating meteorological weather balloons. Accurate thermodynamic modeling of light gases is essential in aerospace and diving applications. Methane has a molar mass of sixteen grams per mole, which is significantly heavier than helium. Nitrogen gas possesses a molar mass of twenty-eight grams per mole, yielding much higher densities. Claiming none of these are correct is false since helium matches the calculated density profile.
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