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Ch.5 - Gases
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.5 - GasesProblema 94
Capitolo 5, Problema 94

Use the van der Waals equation and the ideal gas equation to calculate the pressure exerted by 1.000 mol of Cl2 in a volume of 5.000 L at a temperature of 273.0 K. Explain why the two values are different.

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Identify the given values: n = 1.000 mol, V = 5.000 L, T = 273.0 K, and use the van der Waals constants for Cl2: a = 6.49 L^2 atm/mol^2, b = 0.0562 L/mol.
Use the ideal gas law equation: PV = nRT, where R = 0.0821 L atm/mol K. Substitute the given values to calculate the pressure P.
Use the van der Waals equation: \((P + \frac{an^2}{V^2})(V - nb) = nRT\). Substitute the given values and solve for the pressure P.
Compare the pressures obtained from the ideal gas law and the van der Waals equation. Note that the van der Waals equation accounts for intermolecular forces and the volume occupied by gas molecules, which the ideal gas law does not.
Explain that the difference in calculated pressures arises because the ideal gas law assumes no intermolecular forces and that gas molecules have no volume, while the van der Waals equation provides a more accurate representation by considering these factors.

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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, R is the ideal gas constant, and T is temperature in Kelvin. It assumes that gas particles do not interact and occupy no volume, making it a good approximation for gases under low pressure and high temperature.
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Ideal Gas Law Formula

van der Waals Equation

The van der Waals equation is an adjustment of the Ideal Gas Law that accounts for the volume occupied by gas particles and the attractive forces between them. It is expressed as (P + a(n/V)²)(V - nb) = nRT, where 'a' and 'b' are constants specific to each gas. This equation provides a more accurate description of real gas behavior, especially under high pressure and low temperature.
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Van der Waals Equation

Real vs. Ideal Gases

Real gases deviate from ideal behavior due to intermolecular forces and the finite volume of gas particles. At high pressures and low temperatures, these deviations become significant, leading to differences in calculated pressure using the Ideal Gas Law versus the van der Waals equation. Understanding these differences is crucial for accurately predicting gas behavior in various conditions.
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Ideal Gas Law Formula
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