Ch.10 - Gases

Problem 29b

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Chapter 10, Problem 29b

(b) What is 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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Standard Temperature and Pressure

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Related Practice

Textbook Question

You have a gas at 25 C confined to a cylinder with a movable piston. Which of the following actions would double the gas pressure? (a) Lifting up on the piston to double the volume while keeping the temperature constant (b) Heating the gas so that its temperature rises from 25 C to 50 C, while keeping the volume constant (c) Pushing down on the piston to halve the volume while keeping the temperature constant.

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Textbook Question

(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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Textbook Question

(b) If a car tire is filled to a pressure of 220.6 kPa measured at 24 °C, what will be the tire pressure if the tires heat up to 49 °C during driving?

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Textbook Question

(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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Textbook Question

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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Textbook Question

Suppose you are given two flasks at the same temperature, one of volume 2 L and the other of volume 3 L. The 2-L flask contains 4.8 g of gas, and the gas pressure is x kPa. The 3-L flask contains 0.36 g of gas, and the gas pressure is 0.1x. Do the two gases have the same molar mass? If not, which contains the gas of higher molar mass?

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