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36. How many grams of gaseous boron trifluoride, BF3, are contained in a 4.341-L bulb at 788.0 K if the pressure is 1.220 atm? g BF3

36. How many grams of gaseous boron trifluoride, BF3, are contained in a 4.341-L bulb at 788.0 K if the pressure is 1.220 atm? g BF3

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.128QP: Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do...
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**Problem Statement:** 36. How many *grams* of gaseous boron trifluoride, BF₃, are contained in a 4.341-L bulb at 788.0 K if the pressure is 1.220 atm? **Answer Box:** [ ] g BF₃ **Explanation:** To solve this problem, you would typically use the Ideal Gas Law, which is given by: \[ PV = nRT \] Where: - \( P \) is the pressure (in atm) - \( V \) is the volume (in liters) - \( n \) is the number of moles of the gas - \( R \) is the ideal gas constant (0.0821 L·atm/mol·K) - \( T \) is the temperature (in Kelvin) To find the mass in grams, calculate \( n \) using the above equation and then convert moles to grams using the molar mass of boron trifluoride (BF₃). **Steps:** 1. Substitute the given values into the Ideal Gas Law to find \( n \). 2. Calculate the molar mass of BF₃. 3. Multiply the number of moles by the molar mass to get the mass in grams.
Transcribed Image Text:**Problem Statement:** 36. How many *grams* of gaseous boron trifluoride, BF₃, are contained in a 4.341-L bulb at 788.0 K if the pressure is 1.220 atm? **Answer Box:** [ ] g BF₃ **Explanation:** To solve this problem, you would typically use the Ideal Gas Law, which is given by: \[ PV = nRT \] Where: - \( P \) is the pressure (in atm) - \( V \) is the volume (in liters) - \( n \) is the number of moles of the gas - \( R \) is the ideal gas constant (0.0821 L·atm/mol·K) - \( T \) is the temperature (in Kelvin) To find the mass in grams, calculate \( n \) using the above equation and then convert moles to grams using the molar mass of boron trifluoride (BF₃). **Steps:** 1. Substitute the given values into the Ideal Gas Law to find \( n \). 2. Calculate the molar mass of BF₃. 3. Multiply the number of moles by the molar mass to get the mass in grams.
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