Chapter 14: Problem 55
At a given temperature and pressure, what mathematical relationship exists between the density and molar mass of a gas? Explain your answer.
Short Answer
Expert verified
Density is directly proportional to molar mass when temperature and pressure are constant, as per the equation \( \rho = \frac{PM}{RT} \).
Step by step solution
01
Define the Ideal Gas Law
The Ideal Gas Law 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.
02
Rearrange for Moles (n)
The number of moles \( n \) can be expressed as \( \frac{m}{M} \), where \( m \) is the mass of the gas and \( M \) is the molar mass of the gas. Substitute this into the Ideal Gas Law to get \( PV = \frac{m}{M}RT \).
03
Solve for Density (ρ)
Density \( \rho \) is defined as mass per unit volume, or \( \rho = \frac{m}{V} \). Rearrange the equation from Step 2 to solve for \( m \) as \( m = \rho V \). Substitute into \( PV = \frac{m}{M}RT \), resulting in \( PV = \frac{\rho V}{M}RT \).
04
Simplify the Equation
Cancel out \( V \) from both sides of the equation to obtain \( P = \frac{\rho RT}{M} \).
05
Isolate Density (ρ)
Rearrange the equation from Step 4 to solve for \( \rho \), giving \( \rho = \frac{PM}{RT} \).
06
Express the Relationship Between Density and Molar Mass
The derived equation \( \rho = \frac{PM}{RT} \) shows the relationship between density \( \rho \) and molar mass \( M \). At constant pressure and temperature, density is directly proportional to molar mass.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Density
Density is one of those fundamental concepts in physics and chemistry that can sometimes seem perplexing; however, it can be easily understood with the right explanation. At its core, the density of a gas is a measure of how much mass it has within a certain volume. Mathematically, we express density as \( \rho = \frac{m}{V} \), where \( m \) is the mass and \( V \) is the volume.
Understanding density is particularly important when dealing with gases, which can change their density depending on a variety of factors, such as changes in pressure and temperature. If you increase the pressure of a gas while keeping the temperature constant, the gas particles get compressed, and the density increases since the same amount of mass takes up less space.
Similarly, if the temperature of a gas is increased at constant pressure, the particles spread out more due to increased kinetic energy, thereby decreasing its density as the same mass occupies a larger volume. In the Ideal Gas Law, we can see this manifestation where density \( \rho \) is linked with pressure \( P \), molar mass \( M \), constant \( R \), and temperature \( T \) via the equation \( \rho = \frac{PM}{RT} \). The higher the pressure or molar mass, the greater the density, and vice versa for temperature.
Understanding density is particularly important when dealing with gases, which can change their density depending on a variety of factors, such as changes in pressure and temperature. If you increase the pressure of a gas while keeping the temperature constant, the gas particles get compressed, and the density increases since the same amount of mass takes up less space.
Similarly, if the temperature of a gas is increased at constant pressure, the particles spread out more due to increased kinetic energy, thereby decreasing its density as the same mass occupies a larger volume. In the Ideal Gas Law, we can see this manifestation where density \( \rho \) is linked with pressure \( P \), molar mass \( M \), constant \( R \), and temperature \( T \) via the equation \( \rho = \frac{PM}{RT} \). The higher the pressure or molar mass, the greater the density, and vice versa for temperature.
- Density is mass per unit volume.
- Affected by pressure and temperature changes.
- Important for understanding gas behavior under different conditions.
Molar Mass
Molar mass is another crucial concept when working with gases and their properties. It's essentially the mass of one mole of a substance, usually expressed in grams per mole (g/mol). One mole contains Avogadro's number of molecules or atoms, which is approximately \( 6.022 \times 10^{23} \).
Why is molar mass important in the Ideal Gas Law? Well, it serves as a bridge connecting the number of moles to the actual substance's mass. In our Ideal Gas Law manipulation, we derive that \( n = \frac{m}{M} \), where \( n \) is the number of moles, \( m \) is the mass, and \( M \) is the molar mass. Substitute this into the Ideal Gas Law, and you see how molar mass directly influences other properties like density.
For gases, a higher molar mass means that, at a given pressure and temperature, the density will be higher because more massive molecules occupy a given volume. Therefore, understanding molar mass helps explain why different gases exhibit different densities under the same conditions.
Why is molar mass important in the Ideal Gas Law? Well, it serves as a bridge connecting the number of moles to the actual substance's mass. In our Ideal Gas Law manipulation, we derive that \( n = \frac{m}{M} \), where \( n \) is the number of moles, \( m \) is the mass, and \( M \) is the molar mass. Substitute this into the Ideal Gas Law, and you see how molar mass directly influences other properties like density.
For gases, a higher molar mass means that, at a given pressure and temperature, the density will be higher because more massive molecules occupy a given volume. Therefore, understanding molar mass helps explain why different gases exhibit different densities under the same conditions.
- Molar mass connects mass with moles.
- Crucial for relating gas behavior to mass.
- Directly affects gas density under specific conditions.
Temperature and Pressure
Temperature and pressure are vital factors affecting gas behavior and properties. Temperature is a measure of the average kinetic energy of gas molecules. As temperature increases, molecules move faster, and if the pressure doesn't change, they occupy a larger volume, making the gas less dense.
Pressure, on the other hand, is the force that the gas exerts against the walls of its container, usually measured in Pascals or atmospheres. An increase in pressure means that gas molecules are forced into a smaller space, increasing the density if the temperature remains constant.
The Ideal Gas Law, which is \( PV = nRT \), elegantly describes how these two variables are interwoven with volume and moles of gas. We see that with a constant amount of gas, increasing pressure will reduce volume and increase the density, while increasing temperature will increase volume and reduce density if pressure remains constant.
Understanding the impacts of temperature and pressure on gases helps predict their density and behavior in various scenarios, making this knowledge essential in scientific and engineering applications.
Pressure, on the other hand, is the force that the gas exerts against the walls of its container, usually measured in Pascals or atmospheres. An increase in pressure means that gas molecules are forced into a smaller space, increasing the density if the temperature remains constant.
The Ideal Gas Law, which is \( PV = nRT \), elegantly describes how these two variables are interwoven with volume and moles of gas. We see that with a constant amount of gas, increasing pressure will reduce volume and increase the density, while increasing temperature will increase volume and reduce density if pressure remains constant.
Understanding the impacts of temperature and pressure on gases helps predict their density and behavior in various scenarios, making this knowledge essential in scientific and engineering applications.
- Temperature relates to kinetic energy of molecules.
- Pressure is the force exerted by gas molecules.
- Both affect gas density and behavior.