Question

Explain Which of the three variables that apply to equal amounts of gases are directly proportional? Which are inversely proportional?

Short answer

For equal amounts of gases, temperature (T) is directly proportional to the product of pressure and volume (PV), and pressure (P) is inversely proportional to volume (V). This relationship is based on the Ideal Gas Law, \(PV = nRT\), where n and R are constants.

Step-by-step solution

Ideal Gas Law Formula

The Ideal Gas Law states that \(PV = nRT\). If we need to compare the variables for equal amounts of gases, we have to ensure the number of moles 'n' remains constant. In our case, we will consider n and R as constants.

Direct Proportionality

When one variable increases and the other variable increases as well, they are said to be directly proportional. From the Ideal Gas Law, since n and R are constants, if we increase the temperature (T), the product of pressure and volume (PV) must also increase to keep the equation balanced. Therefore, for equal amounts of gases, temperature (T) is directly proportional to the product of pressure and volume (PV).

Inverse Proportionality

When one variable increases and the other variable decreases, they are said to be inversely proportional. As we know, T is directly proportional to PV. Now, if we assume that temperature (T) remains constant, as the pressure (P) increases, the volume (V) must decrease to keep the product PV constant. Therefore, for equal amounts of gases, pressure (P) is inversely proportional to volume (V), and vice versa. In conclusion, for equal amounts of gases, temperature is directly proportional to the product of pressure and volume, and pressure is inversely proportional to volume.

Key concepts

Direct Proportionality

Understanding the concept of direct proportionality is pivotal in mastering various scientific and mathematical principles. When two variables are directly proportional, as one increases, the other increases at the same rate. In the context of gas laws, this relationship is observed between the temperature of a gas and its pressure-volume product.

For example, with the Ideal Gas Law formula, \(PV = nRT\), holding the number of moles (n) and the gas constant (R) constant, an increase in temperature (T) will result in an equal increase in the product of pressure (P) and volume (V). This is because the formula dictates that for temperature to go up, the PV must also rise to maintain equilibrium in the equation. This direct relationship helps us to predict and understand the behavior of gases under different thermal conditions.

Inverse Proportionality

In contrast to direct proportionality, inverse proportionality describes a relationship where one variable increases as the other decreases. When studying gases, this concept becomes particularly relevant when temperature remains constant.

If we look at the same Ideal Gas Law, \(PV = nRT\), and keep both the temperature (T) and the amount of gas (n) constant, we discover that if the pressure (P) of the gas goes up, the volume (V) must come down in order to maintain the constant value of PV. This inverse relationship between pressure and volume affords us the ability to foretell how gases will adapt when subjected to changing pressures within the same temperature, a principle known as Boyle's Law.

Gas Laws

Gas laws are simplified models that predict and describe the behavior of gases under different conditions. These laws are built upon concepts of direct and inverse proportionality, integrating them to form the foundational principles of gas behavior.

Boyle's Law and Charles's Law

Boyle’s Law highlights the inverse proportionality between pressure and volume at constant temperature, while Charles’s Law showcases the direct relationship between volume and temperature at constant pressure. Also integral to the gas laws is Avogadro's Law, which posits that volume is directly proportional to the number of moles at constant temperature and pressure.

Combining Gas Laws

The Ideal Gas Law is a comprehensive equation that unites Boyle's, Charles's, and Avogadro's laws, by indicating the relationship between pressure, volume, temperature, and the number of moles of the gas.

Pressure-Volume Relationship

Understanding the pressure-volume relationship is essential when dealing with gases, as it helps in predicting how changes in one will affect the other. It's a classic example of inverse proportionality.

The Ideal Gas Law presents this relationship algebraically, but Boyle's Law, a specific case of the Ideal Gas Law, gives it a more focused exposition. For a given mass of gas at a constant temperature (assuming ideal behavior), the pressure exerted by the gas is inversely proportional to its volume. This means that if you compress a gas (decreasing its volume), its pressure will increase, provided the temperature doesn't change. Such predictable behavior is crucial in myriad applications, from designing syringes to engineering the engines of cars.