(b) What is the molar volume of an ideal gas at STP?

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Recall the definition of Standard Temperature and Pressure (STP), which is a temperature of 273.15 K (0°C) and a pressure of 1 atm.

Understand that the molar volume is the volume occupied by one mole of any gas at STP.

Use the Ideal Gas Law equation, which is PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.

Substitute the values for STP into the Ideal Gas Law equation: P = 1 atm, n = 1 mole, R = 0.0821 L atm / K mol (the value of the gas constant in these units), and T = 273.15 K.

Solve for V, the volume, to find the molar volume of an ideal gas at STP.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Volume

Molar volume is the volume occupied by one mole of a substance at a given temperature and pressure. For gases, it is typically expressed in liters per mole (L/mol). Understanding molar volume is crucial for relating the amount of gas to its physical space, especially in stoichiometric calculations.

Ideal Gas Law

The Ideal Gas Law is a fundamental equation in chemistry that relates the pressure, volume, temperature, and number of moles of an ideal gas. It is expressed as PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. This law helps predict the behavior of gases under various conditions.

Standard Temperature and Pressure (STP)

Standard Temperature and Pressure (STP) is a reference point used in chemistry defined as 0 degrees Celsius (273.15 K) and 1 atmosphere (atm) of pressure. At STP, the molar volume of an ideal gas is approximately 22.4 liters. This standardization allows for consistent calculations and comparisons in gas behavior.

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(c) Room temperature is often assumed to be 25 °C. Calculate the molar volume of an ideal gas at 25 °C and 101.3 kPa pressure.

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(a) Amonton's law expresses the relationship between pressure and temperature. Use Charles's law and Boyle's law to derive the proportionality relationship between P and T.

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(d) If you measure pressure in bars instead of atmospheres, calculate the corresponding value of R in L-bar/mol-K.

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Suppose you are given two 2-L flasks and told that one contains a gas of molar mass 28, the other a gas of molar mass 56, both at the same temperature and pressure. The mass of gas in the flask A is 1.0 g and the mass of gas in the flask B is 2.0 g. Which flask contains the gas of molar mass 28, and which contains the gas of molar mass 56?

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