Boron trifluoride gas is collected at −10.0°C in an evacuated flask with a measured volume of 40.0L. When all the gas has been collected, the pressure in the flask is measured to be 0.470atm .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.
Question
Boron trifluoride gas is collected at −10.0°C in an evacuated flask with a measured volume of 40.0L. When all the gas has been collected, the pressure in the flask is measured to be 0.470atm .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.
Solution
To solve this problem, we will use the ideal gas law equation, which is 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, -10.0°C = -10.0 + 273.15 = 263.15 K.
Step 2: Substitute the given values into the ideal gas law equation. The pressure P is 0.470 atm, the volume V is 40.0 L, the ideal gas constant R is 0.0821 L·atm/K·mol (this is the value of R that should be used when pressure is in atm and volume is in liters), and the temperature T is 263.15 K. So, we have 0.470 atm * 40.0 L = n * 0.0821 L·atm/K·mol * 263.15 K.
Step 3: Solve the equation for n, the number of moles. n = (0.470 atm * 40.0 L) / (0.0821 L·atm/K·mol * 263.15 K) = 0.681 mol.
Step 4: To find the mass of boron trifluoride gas collected, we need to multiply the number of moles by the molar mass of boron trifluoride (BF3). The molar mass of BF3 is approximately 67.81 g/mol. So, the mass is 0.681 mol * 67.81 g/mol = 46.2 g.
So, the mass of boron trifluoride gas collected is 46.2 g and the number of moles is 0.681 mol.
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