Boron trifluoride gas is collected at 25.0°C in an evacuated flask with a measured volume of 50.0L. When all the gas has been collected, the pressure in the flask is measured to be 0.400atm .Calculate the mass and number of moles of boron trifluoride gas that were collected. Be sure your answer has the correct number of significant digits.mass: gmole: mol
Question
Boron trifluoride gas is collected at 25.0°C in an evacuated flask with a measured volume of 50.0L. When all the gas has been collected, the pressure in the flask is measured to be 0.400atm .Calculate the mass and number of moles of boron trifluoride gas that were collected. Be sure your answer has the correct number of significant digits.mass: gmole: mol
Solution
To solve this problem, we will use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Step 1: Convert the temperature from Celsius to Kelvin. The formula to convert Celsius to Kelvin is K = °C + 273.15. So, 25.0°C = 25.0 + 273.15 = 298.15 K.
Step 2: Substitute the given values into the ideal gas law equation. We know that P = 0.400 atm, V = 50.0 L, R = 0.0821 L.atm/(mol.K) (this is the value of R when pressure is in atm and volume is in liters), and T = 298.15 K. We want to solve for n, the number of moles.
0.400 atm * 50.0 L = n * 0.0821 L.atm/(mol.K) * 298.15 K
Step 3: Solve for n.
n = (0.400 atm * 50.0 L) / (0.0821 L.atm/(mol.K) * 298.15 K) = 0.816 moles
Step 4: To find the mass, we need to multiply the number of moles by the molar mass of boron trifluoride (BF3). The molar mass of BF3 = 10.81 g/mol (B) + 3*18.998 g/mol (F) = 67.805 g/mol.
mass = n * molar mass = 0.816 moles * 67.805 g/mol = 55.3 g
So, the mass of boron trifluoride gas collected is 55.3 g and the number of moles is 0.816 mol.
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