A given gas has a density measuring 1.964 g dm-3 at 273 K and 76 cm Hg pressure, identifying the gas as _________?
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Answer: B. CO2
Explanation
Using the ideal gas law, a gas with a density of 1.964 g dm^-3 at STP corresponds to carbon dioxide. Dividing mass density by molar volume at standard temperature and pressure yields the correct molar mass. Carbon dioxide has a molecular weight of approximately forty-four grams per mole, matching this density. Gas density depends directly on temperature, pressure, and the molar mass of the molecular substance. Standard temperature and pressure are defined as 273 Kelvin and 76 centimeters of mercury pressure. The ideal gas law relates pressure, volume, temperature, and moles for simplified theoretical calculations.
Analytical chemistry uses density measurements to help identify unknown gases collected during experiments. Environmental scientists monitor carbon dioxide density and concentrations in atmospheric research studies. Industrial chemical processes rely on gas laws to calculate storage tank capacities and flow rates. Methane has a significantly lower molar mass and density than the value specified for carbon dioxide. Ethylene possesses a different molecular weight that yields a lower gas density at standard conditions. Xenon is a heavy noble gas whose density far exceeds the value calculated for this gas sample.
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