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Ch.6 - Gases
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 5th EditionCh.6 - GasesProblema 49
Capitolo 6, Problema 49

Which gas sample has the greatest pressure? Assume that all the samples are at the same temperature. Explain.
Four flasks showing gas particles; varying densities illustrate pressure differences.

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Identify that pressure is directly related to the number of gas particles in a given volume, according to the ideal gas law (PV = nRT).
Observe the four flasks labeled a, b, c, and d, and note the number of gas particles in each flask.
Compare the density of gas particles in each flask visually.
Determine that the flask with the highest density of gas particles will have the greatest pressure, assuming all other conditions (temperature and volume) are constant.
Conclude which flask has the greatest pressure based on the visual comparison of particle density.

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Gas Pressure

Gas pressure is defined as the force exerted by gas particles colliding with the walls of their container. It is influenced by the number of particles, their speed, and the volume of the container. According to the ideal gas law, pressure increases with more gas particles in a given volume, assuming temperature remains constant.
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Pressure Units

Ideal Gas Law

The ideal gas law is a fundamental equation in chemistry represented as PV = nRT, where P is pressure, V is volume, n is the number of moles of gas, R is the ideal gas constant, and T is temperature. This law helps predict the behavior of gases under various conditions and indicates that at constant temperature, pressure is directly proportional to the number of gas particles.
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Ideal Gas Law Formula

Density of Gas

The density of a gas is defined as its mass per unit volume. In the context of gas samples, a higher density often indicates a greater number of gas particles in a given volume, which can lead to higher pressure. When comparing gas samples at the same temperature, the sample with the highest density will typically exert the greatest pressure.
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Gas Density Example
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A 1.0-L container of liquid nitrogen is kept in a closet measuring 1.0 m by 1.0 m by 2.0 m. Assuming that the container is completely full, that the temperature is 25.0 °C, and that the atmospheric pressure is 1.0 atm, calculate the percent (by volume) of air that is displaced if all of the liquid nitrogen evaporates. (Liquid nitrogen has a density of 0.807 g/mL.)

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This picture represents a sample of gas at a pressure of 1 atm, a volume of 1 L, and a temperature of 25 °C. Draw a similar picture showing what would happen to the sample if the volume were reduced to 0.5 L and the temperature were increased to 250 °C. What would happen to the pressure?

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Aerosol cans carry clear warnings against incineration because of the high pressures that can develop upon heating. Suppose that a can contains a residual amount of gas at a pressure of 755 mmHg and a temperature of 25 °C. What would the pressure be if the can were heated to 1155 °C?

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