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Chapter 10: Problem 83

(a) List two experimental conditions under which gases deviate from ideal behavior. (b) List two reasons why the gases deviate from ideal behavior. (c) Explain how the function \(P V / R T\) can be used to show how gases behave nonideally.

Short Answer

Expert verified
(a) Gases deviate from ideal behavior under high pressure and low temperature conditions. (b) Deviation occurs due to intermolecular forces and the actual volume occupied by gas particles. (c) The function \(PV/RT\) can be used to show nonideal behavior, as gases with a value that deviates from \(1\) indicate nonideality.

Step by step solution

01

(a) Explain Two Experimental Conditions Under Which Gases Deviate from Ideal Behavior

There are several experimental conditions that lead to deviation from ideal behavior. Here are two such conditions: 1. High pressure: Gases deviate from ideal behavior when the pressure is high because under high pressure conditions, the gas particles are pushed closer together, causing particle interactions and volume occupancies that were initially negligible to become significant. 2. Low temperature: Deviation from ideal behavior is observed at low temperatures because, as the temperature decreases, gas particles move more slowly and have more time to interact. These interactions between gas particles become more apparent at lower temperatures.
02

(b) List Two Reasons Why Gases Deviate from Ideal Behavior

Gases deviate from ideal behavior for various reasons. Here are two significant factors: 1. Intermolecular forces: At high pressure and low temperature, the intermolecular forces between gas particles become more pronounced and affect the gas' behavior. These molecular forces are not taken into account in the ideal gas law, causing deviations. 2. Particle size: In the ideal gas law, gas particles are assumed to have negligible volume. However, as pressure increases and/or temperature decreases, the volume occupied by the gas particles can no longer be considered negligible, leading to deviations from ideal behavior.
03

(c) Explain How the Function \(PV/RT\) Can Be Used to Show How Gases Behave Nonideally

The function \(PV/RT\) is derived from the ideal gas law, where \(P\) represents pressure, \(V\) represents volume, \(n\) represents the number of moles, \(R\) is the ideal gas constant, and \(T\) is the temperature. In an ideal gas, the value of \(PV/RT = 1\). However, a gas that does not follow ideal behavior will have a \(PV/RT\) value that deviates from \(1\). The deviation of the ratio from 1 indicates the degree of nonideality of the gas. By comparing the \(PV/RT\) values of different gases under various conditions (e.g., high pressure or low temperature), we can determine the extent to which a particular gas deviates from ideal behavior. Additionally, comparing these values can help us understand the effects of particle size and intermolecular forces on the gas' behavior.

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Most popular questions from this chapter

Large amounts of nitrogen gas are used in the manufacture of ammonia, principally for use in fertilizers. Suppose \(120.00 \mathrm{~kg}\) of \(\mathrm{N}_{2}(g)\) is stored in a 1100.0-L metal cylinder at \(280^{\circ} \mathrm{C}\). (a) Calculate the pressure of the gas, assuming ideal-gas behavior. (b) By using data in Table 10.3, calculate the pressure of the gas according to the van der Waals equation. (c) Under the conditions of this problem, which correction dominates, the one for finite volume of gas molecules or the one for attractive interactions?

Newton had an incorrect theory of gases in which he assumed that all gas molecules repel one another and the walls of their container. Thus, the molecules of a gas are statically and uniformly distributed, trying to get as far apart as possible from one another and the vessel walls. This repulsion gives rise to pressure. Explain why Charles's law argues for the kinetic- molecular theory and against Newton's model.

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A fixed quantity of gas at \(21^{\circ} \mathrm{C}\) exhibits a pressure of 752 torr and occupies a volume of \(4.38 \mathrm{~L}\). (a) Use Boyle's law to calculate the volume the gas will occupy if the pressure is increased to \(1.88\) atm while the temperature is held constant. (b) Use Charles's law to calculate the volume the gas will occupy if the temperature is increased to \(175^{\circ} \mathrm{C}\) while the pressure is held constant.
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