Problem 34 - Chemistry

Question

A certain amount of gas at \(25^{\circ} \mathrm{C}\) and at a pressure of 0.800 atm is contained in a glass vessel. Suppose that the vessel can withstand a pressure of 2.00 atm. How high can you raise the temperature of the gas without bursting the vessel?

Step-by-Step Solution

Answer

The maximum temperature the gas can reach without breaking the vessel is approximately \(745^{\circ} \mathrm{C}\) or \(1018.19 \mathrm{K}\).

Step 1: Understand the Problem and Organize the Information

Identify and record what information is known from the problem. We have the initial temperature \(T_1 = 25^{\circ} \mathrm{C} = 298.15 \mathrm{K} \) (converted to Kelvin), the initial pressure \(P_1 = 0.800 \mathrm{atm}\), and the final pressure \(P_2 = 2.00 \mathrm{atm}\). We are looking for the final temperature \(T_2\).

Step 2: Apply the Ideal Gas Law Ratio

We can use a ratio derived from the ideal gas law \(P_1/T_1 = P_2/T_2\). Substitute the known values, and solve for the unknown final temperature \(T_2\). So, \(T_2 = P_2 *T_1 / P_1 = 2.00 \mathrm{atm} * 298.15 \mathrm{K} / 0.800 \mathrm{atm}\).

Step 3: Solve for the Unknown

Calculate the value of \(T_2\), which represents the maximum temperature that can be reached without breaking the vessel. Remember to convert back to Celsius if necessary.

Key Concepts

Gas Temperature Pressure Relationship

Understanding the relationship between gas temperature and pressure is central to predicting how a gas will behave under varying conditions. According to the ideal gas law, for a given amount of gas at a constant volume, the pressure of the gas is directly proportional to its temperature in Kelvin. This means if you raise the temperature of a gas, its pressure tends to increase, provided the volume is held constant.

This is precisely what the problem in the exercise explores. As the temperature of the gas in the vessel increases, the pressure inside the vessel also increases. The exercise asks how high we can raise the temperature before reaching a pressure that the vessel can no longer withstand. The ideal gas law, specifically the ratio \(P_1/T_1 = P_2/T_2\), allows us to find this maximum temperature.

Real-world applications of this principle are abundant. For example, it's crucial for understanding the workings of internal combustion engines and refrigeration systems. This concept is not only foundational in understanding gas behavior but also illustrates the importance of temperature and pressure control in various technologies.

Kelvin Temperature Scale

The Kelvin scale is an absolute temperature scale, meaning it starts from absolute zero, which is the coldest possible temperature where particles have minimal thermal motion. Unlike Celsius or Fahrenheit, Kelvin does not use degrees and is fundamental in scientific research and calculations.

In chemistry and physics, particularly when using the ideal gas law, temperatures must be converted into Kelvin to ensure accuracy. This is because the Kelvin scale is directly related to the energy of particles. The problem provided required the conversion of the initial temperature from Celsius to Kelvin, which can be carried out by adding 273.15 to the Celsius temperature.

The step-by-step solution of our exercise includes this conversion with \(25^\circ \textrm{C} = 298.15 \textrm{K}\). The significance of using Kelvin becomes evident when we apply gas laws, as it assures the proportionality between temperature and other variables such as pressure and volume.

Gas Laws in Chemistry

Gas laws in chemistry are a collection of laws that describe how gases behave and how they respond to changes in temperature, volume, and pressure. The ideal gas law, which is represented by the equation \(PV=nRT\), is a cornerstone in this topic and combines several other laws such as Boyle's Law (pressure-volume relationship), Charles's Law (volume-temperature relationship), and Gay-Lussac's Law (pressure-temperature relationship).

These laws are simplified models that assume gases behave ideally. While real gases exhibit ideal behavior under certain conditions (low pressure and high temperature), they can deviate at high pressures and low temperatures. However, for many practical cases and especially in educational settings, the ideal gas law provides a close approximation of gas behavior.

The exercise we analyzed uses the ideal gas law to find the temperature limit before a gas vessel is compromised. Mastery of these laws is essential for anyone studying chemistry or physics as they're not simply academic exercises but tools for understanding and predicting the behavior of gases in practical situations.