Not converting temperature to Kelvin

Oct 13, 2025 by recoveryshake.com 23 views

What is the Pressure in atm of a 5.00 L Tank with 2.50 moles of Oxygen at $39.3^{\circ} C$ ?

Understanding the Ideal Gas Law

The ideal gas law is a fundamental concept in chemistry that describes the behavior of gases under various conditions. It is expressed by the equation: PV = nRT, where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the gas constant, and T is the temperature of the gas in Kelvin. In this article, we will use the ideal gas law to calculate the pressure in atm of a 5.00 L tank with 2.50 moles of oxygen at $39.3^{\circ} C$ .

Converting Temperature to Kelvin

Before we can use the ideal gas law, we need to convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is: T(K) = T(°C) + 273.15. Plugging in the given temperature, we get: T(K) = 39.3 + 273.15 = 312.45 K.

Rearranging the Ideal Gas Law

To solve for pressure, we need to rearrange the ideal gas law equation to isolate P. We can do this by dividing both sides of the equation by V: P = nRT/V. Now we have the equation in terms of pressure.

Plugging in the Values

Now that we have the equation in terms of pressure, we can plug in the given values: n = 2.50 moles, R = 0.08206 L atm/mol K, T = 312.45 K, and V = 5.00 L. Plugging in these values, we get: P = (2.50 mol)(0.08206 L atm/mol K)(312.45 K)/(5.00 L).

Calculating the Pressure

Now we can calculate the pressure by evaluating the expression: P = (2.50 mol)(0.08206 L atm/mol K)(312.45 K)/(5.00 L) = 12.63 atm.

Conclusion

In this article, we used the ideal gas law to calculate the pressure in atm of a 5.00 L tank with 2.50 moles of oxygen at $39.3^{\circ} C$ . We first converted the temperature from Celsius to Kelvin, then rearranged the ideal gas law equation to isolate P, and finally plugged in the given values to calculate the pressure. The result is a pressure of 12.63 atm.

Understanding the Significance of Pressure

Pressure is an important concept in chemistry that has many practical applications. In the context of the ideal gas law, pressure is a measure of the force exerted by a gas on its container. In this article, we saw how to calculate the pressure of a gas using the ideal gas law. This is a fundamental concept in chemistry that has many real-world applications, such as in the design of gas tanks and pipelines.

Real-World Applications of Pressure

Pressure is an important concept in many real-world applications, including:

Gas Tanks and Pipelines: Pressure is a critical factor in the design of gas tanks and pipelines. It determines the amount of gas that can be stored or transported, and it affects the safety of the system.
Scuba Diving: Pressure is a critical factor in scuba diving. Divers must be aware of the pressure of the water they are diving in, and they must take steps to avoid decompression sickness.
Industrial Processes: Pressure is a critical factor in many industrial processes, including the production of chemicals and the operation of power plants.

Conclusion

In conclusion, pressure is an important concept in chemistry that has many practical applications. In this article, we used the ideal gas law to calculate the pressure in atm of a 5.00 L tank with 2.50 moles of oxygen at $39.3^{\circ} C$ . We saw how to convert the temperature from Celsius to Kelvin, rearrange the ideal gas law equation to isolate P, and plug in the given values to calculate the pressure. The result is a pressure of 12.63 atm. This is a fundamental concept in chemistry that has many real-world applications, and it is an important tool for chemists and engineers.

References

Ideal Gas Law: The ideal gas law is a fundamental concept in chemistry that describes the behavior of gases under various conditions. It is expressed by the equation: PV = nRT, where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the gas constant, and T is the temperature of the gas in Kelvin.
Gas Constant: The gas constant is a fundamental constant in chemistry that is used in the ideal gas law equation. It is expressed by the equation: R = 0.08206 L atm/mol K.
Temperature Conversion: Temperature conversion is an important concept in chemistry that involves converting temperatures from one unit to another. In this article, we converted the temperature from Celsius to Kelvin using the formula: T(K) = T(°C) + 273.15.

Further Reading

Ideal Gas Law: The ideal gas law is a fundamental concept in chemistry that describes the behavior of gases under various conditions. It is expressed by the equation: PV = nRT, where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the gas constant, and T is the temperature of the gas in Kelvin.
Gas Constant: The gas constant is a fundamental constant in chemistry that is used in the ideal gas law equation. It is expressed by the equation: R = 0.08206 L atm/mol K.
Temperature Conversion: Temperature conversion is an important concept in chemistry that involves converting temperatures from one unit to another. In this article, we converted the temperature from Celsius to Kelvin using the formula: T(K) = T(°C) + 273.15.
Q&A: Understanding the Ideal Gas Law and Pressure

Frequently Asked Questions

In this article, we will answer some frequently asked questions about the ideal gas law and pressure. These questions cover a range of topics, from the basics of the ideal gas law to more advanced concepts like pressure and temperature.

Q: What is the ideal gas law?

A: The ideal gas law is a fundamental concept in chemistry that describes the behavior of gases under various conditions. It is expressed by the equation: PV = nRT, where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the gas constant, and T is the temperature of the gas in Kelvin.

Q: What is the gas constant?

A: The gas constant is a fundamental constant in chemistry that is used in the ideal gas law equation. It is expressed by the equation: R = 0.08206 L atm/mol K.

Q: How do I convert temperature from Celsius to Kelvin?

A: To convert temperature from Celsius to Kelvin, you can use the formula: T(K) = T(°C) + 273.15. For example, if the temperature is 25°C, the temperature in Kelvin would be 298.15 K.

Q: What is pressure?

A: Pressure is a measure of the force exerted by a gas on its container. It is an important concept in chemistry that has many practical applications.

Q: How do I calculate pressure using the ideal gas law?

A: To calculate pressure using the ideal gas law, you can rearrange the equation to isolate P: P = nRT/V. Then, you can plug in the given values and solve for P.

Q: What are some real-world applications of pressure?

A: Pressure is an important concept in many real-world applications, including:

Gas Tanks and Pipelines: Pressure is a critical factor in the design of gas tanks and pipelines. It determines the amount of gas that can be stored or transported, and it affects the safety of the system.
Scuba Diving: Pressure is a critical factor in scuba diving. Divers must be aware of the pressure of the water they are diving in, and they must take steps to avoid decompression sickness.
Industrial Processes: Pressure is a critical factor in many industrial processes, including the production of chemicals and the operation of power plants.

Q: What are some common mistakes to avoid when working with the ideal gas law?

A: Some common mistakes to avoid when working with the ideal gas law include:

Not converting temperature to Kelvin: Make sure to convert temperature to Kelvin before using the ideal gas law equation.
Not using the correct units: Make sure to use the correct units for pressure, volume, and temperature.
Not checking the units of the gas constant: Make sure to check the units of the gas constant to ensure that they match the units of the other variables.

Q: What are some advanced concepts related to the ideal gas law?

A: Some advanced concepts related to the ideal gas law include:

Non-ideal gases: Non-ideal gases are gases that do not behave according to the ideal gas law. They may exhibit non-ideal behavior due to intermolecular forces or other factors.
Gas mixtures: Gas mixtures are mixtures of two or more gases. They can be modeled using the ideal gas law, but they may exhibit non-ideal behavior due to interactions between the different gases.
High-pressure gases: High-pressure gases are gases that are subjected to high pressures. They may exhibit non-ideal behavior due to the effects of pressure on the gas molecules.

Conclusion

In this article, we have answered some frequently asked questions about the ideal gas law and pressure. These questions cover a range of topics, from the basics of the ideal gas law to more advanced concepts like pressure and temperature. We hope that this article has been helpful in clarifying some of the common misconceptions and misunderstandings about the ideal gas law and pressure.