According to Avogadro’s Hypothesis, what is true regarding gas molecules ______________________?
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Answer: A. the molecular weights of all the perfect gases occupy the same volume under same conditions of pressure and temperature
Explanation
Avogadro hypothesis states that equal volumes of all perfect gases under identical pressure and temperature contain equal molecules. This fundamental gas law establishes that molecular weights of perfect gases occupy identical volumes under standard conditions. It provides the basis for connecting macroscopic gas volumes to microscopic molecular counts. Amedeo Avogadro first proposed this principle, leading to the universal constant known as Avogadro number. Ideal gas behavior assumes negligible molecular volume and absence of intermolecular attractive forces. One mole of any ideal gas occupies approximately twenty two point four liters at standard temperature and pressure.
Chemical engineers use Avogadro law extensively when calculating stoichiometric gas proportions in combustion reactions. Thermodynamic property tables rely on molar mass relationships derived from ideal gas hypotheses. Understanding gas volumes helps in designing ventilation systems and chemical processing reactors safely. Dalton law of partial pressures states that total pressure equals the sum of individual gas pressures. Products of gas constants and molecular weights define specific gas constant relationships rather than volume counts. Stating that gases have two specific heats describes thermodynamic properties rather than Avogadro hypothesis.
- Subject
- Engineering
- Category
- Mechanical Engineering
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- —
- Difficulty
- medium
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