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Which gas sample has the greatest volume at STP?
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11 Gases
Standard Temperature and Pressure
2:33 minutiProblema 70
Domanda del libro di testo
How many molecules are in 1.0 L of O₂ at STP? How may grams of O₂?
Guida verificata passo dopo passo1
Identify that the problem involves calculating the number of molecules and grams of O₂ at Standard Temperature and Pressure (STP).
Recall that at STP, 1 mole of any gas occupies 22.4 L. Therefore, determine the number of moles of O₂ in 1.0 L by using the formula: \( \text{moles of O}_2 = \frac{1.0 \text{ L}}{22.4 \text{ L/mol}} \).
Use Avogadro's number, \(6.022 \times 10^{23}\) molecules/mol, to calculate the number of molecules in the moles of O₂ obtained from the previous step.
To find the mass of O₂, use the molar mass of O₂, which is approximately 32.00 g/mol. Multiply the number of moles of O₂ by the molar mass to find the mass in grams.
Summarize the steps: Calculate moles from volume using STP conditions, convert moles to molecules using Avogadro's number, and convert moles to grams using the molar mass of O₂.
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Molar Volume at STP
At Standard Temperature and Pressure (STP), one mole of any ideal gas occupies a volume of 22.4 liters. This concept is crucial for converting between the volume of a gas and the number of moles, allowing us to determine how many molecules are present in a given volume.
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00:53
Molarity
Avogadro's Number
Avogadro's number, approximately 6.022 x 10²³, represents the number of molecules in one mole of a substance. This constant is essential for converting moles of a gas into the actual number of molecules, which is necessary for answering the first part of the question regarding the number of molecules in 1.0 L of O₂.
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Molar Mass of O₂
The molar mass of O₂ (oxygen gas) is approximately 32 grams per mole, calculated from the atomic mass of oxygen. This concept is important for converting moles of O₂ into grams, which is needed to answer the second part of the question about how many grams of O₂ are present in 1.0 L at STP.
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01:10Calculating Molar Mass
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