Calculating the Number of Moles of BF3

Oct 13, 2025 by miodeya.com 77 views

How Many Grams of Gaseous Boron Trifluoride are Contained in a 4.3410-L Bulb?

Understanding the Problem

To determine the amount of gaseous boron trifluoride (BF3) contained in a 4.3410-L bulb at 788.0 K and 1.220 atm, we need to apply the ideal gas law. The ideal gas law is a fundamental principle in chemistry that relates the pressure, volume, and temperature of a gas. The equation is given by:

PV = nRT

where:

P is the pressure of the gas in atmospheres (atm)
V is the volume of the gas in liters (L)
n is the number of moles of the gas
R is the gas constant in L atm/mol K
T is the temperature of the gas in Kelvin (K)

Calculating the Number of Moles of BF3

To find the number of moles of BF3, we can rearrange the ideal gas law equation to solve for n:

n = PV / RT

We are given the following values:

P = 1.220 atm
V = 4.3410 L
R = 0.08206 L atm/mol K
T = 788.0 K

Substituting these values into the equation, we get:

n = (1.220 atm * 4.3410 L) / (0.08206 L atm/mol K * 788.0 K)

n = 0.1833 mol

Calculating the Mass of BF3

To find the mass of BF3, we need to know the molar mass of BF3. The molar mass of BF3 is 67.74 g/mol.

We can calculate the mass of BF3 by multiplying the number of moles by the molar mass:

mass = n * molar mass

Substituting the values, we get:

mass = 0.1833 mol * 67.74 g/mol

mass = 12.41 g

Therefore, the amount of gaseous boron trifluoride (BF3) contained in a 4.3410-L bulb at 788.0 K and 1.220 atm is 12.41 grams.

Conclusion

In this problem, we applied the ideal gas law to determine the number of moles of BF3 contained in a 4.3410-L bulb at 788.0 K and 1.220 atm. We then used the molar mass of BF3 to calculate the mass of the gas. The result shows that the amount of gaseous boron trifluoride (BF3) contained in the bulb is 12.41 grams.

References

Ideal Gas Law: PV = nRT
Molar Mass of BF3: 67.74 g/mol
Gas Constant: 0.08206 L atm/mol K

Additional Information

The ideal gas law is a fundamental principle in chemistry that relates the pressure, volume, and temperature of a gas.
The molar mass of a substance is the mass of one mole of the substance.
The gas constant is a constant that relates the pressure, volume, and temperature of a gas.
Frequently Asked Questions (FAQs) About the Ideal Gas Law and Boron Trifluoride (BF3)

Q: What is the ideal gas law?

A: The ideal gas law is a fundamental principle in chemistry that relates the pressure, volume, and temperature of a gas. The equation is given by:

PV = nRT

where:

P is the pressure of the gas in atmospheres (atm)
V is the volume of the gas in liters (L)
n is the number of moles of the gas
R is the gas constant in L atm/mol K
T is the temperature of the gas in Kelvin (K)

Q: What is the molar mass of boron trifluoride (BF3)?

A: The molar mass of BF3 is 67.74 g/mol.

Q: How do I calculate the number of moles of a gas using the ideal gas law?

A: To calculate the number of moles of a gas using the ideal gas law, you can rearrange the equation to solve for n:

n = PV / RT

Substitute the given values for P, V, R, and T into the equation to find the number of moles.

Q: What is the gas constant (R)?

A: The gas constant (R) is a constant that relates the pressure, volume, and temperature of a gas. The value of R is 0.08206 L atm/mol K.

Q: How do I calculate the mass of a gas using the molar mass and the number of moles?

A: To calculate the mass of a gas using the molar mass and the number of moles, you can multiply the number of moles by the molar mass:

mass = n * molar mass

Substitute the values for n and the molar mass into the equation to find the mass.

Q: What is the relationship between the ideal gas law and the molar mass of a gas?

A: The ideal gas law and the molar mass of a gas are related in that the ideal gas law can be used to calculate the number of moles of a gas, and the molar mass can be used to calculate the mass of the gas.

Q: Can the ideal gas law be used to calculate the pressure, volume, or temperature of a gas?

A: Yes, the ideal gas law can be used to calculate the pressure, volume, or temperature of a gas, as long as the other two values are known.

Q: What are some common applications of the ideal gas law?

A: The ideal gas law has many common applications in chemistry and physics, including:

Calculating the number of moles of a gas
Calculating the mass of a gas
Calculating the pressure, volume, or temperature of a gas
Understanding the behavior of gases in different conditions

Q: What are some limitations of the ideal gas law?

A: The ideal gas law has some limitations, including:

It assumes that the gas is ideal, meaning that it does not interact with other molecules
It assumes that the gas is in a state of equilibrium
It does not take into account the behavior of gases at very high or very low temperatures

Conclusion

In this article, we have answered some frequently asked questions about the ideal gas law and boron trifluoride (BF3). We have discussed the ideal gas law, the molar mass of BF3, and how to calculate the number of moles and mass of a gas using the ideal gas law. We have also discussed some common applications and limitations of the ideal gas law.