Which sample contains more molecules: 1.00 L of O2 at STP, 1.00 L of air at STP, or 1.00 L of H2 at STP?

검증된 단계별 안내

Understand that at Standard Temperature and Pressure (STP), 1 mole of any ideal gas occupies 22.4 L.

Recognize that the number of molecules in a gas sample is directly proportional to the number of moles of the gas.

Since all samples are 1.00 L and at STP, calculate the number of moles for each gas using the formula: \( \text{moles} = \frac{\text{volume (L)}}{22.4 \text{ L/mol}} \).

Apply the formula to each gas: O2, air, and H2, to find the number of moles in each 1.00 L sample.

Compare the number of moles for each gas to determine which sample contains more molecules, as more moles mean more molecules.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Avogadro's Law

Avogadro's Law states that equal volumes of gases, at the same temperature and pressure, contain an equal number of molecules. This principle is fundamental in determining the number of molecules in a given volume of gas, allowing us to compare different gases under identical conditions.

Standard Temperature and Pressure (STP)

Standard Temperature and Pressure (STP) is defined as a temperature of 0 degrees Celsius (273.15 K) and a pressure of 1 atmosphere (atm). At STP, one mole of any ideal gas occupies a volume of 22.4 liters, which is crucial for calculating the number of moles and, consequently, the number of molecules in a gas sample.

Composition of Air

Air is primarily composed of nitrogen (approximately 78%), oxygen (about 21%), and trace amounts of other gases, including argon and carbon dioxide. When comparing the number of molecules in 1.00 L of air to pure gases like O2 and H2, it is essential to consider the molar composition of air, as it affects the total number of molecules present in the same volume.