A reaction at 11.0°C produces 133 mmol of boron trifluoride gas. Calculate the volume of the collected boron trifluoride gas, assuming the room pressure is exactly 1 atm. Round your answer to three significant digits.

To calculate the volume of the boron trifluoride (BF3) gas produced, we can use the Ideal Gas Law, which is given by the equation PV = nRT, where:

- P is the pressure, - V is the volume, - n is the number of moles of gas, - R is the ideal gas constant, - T is the temperature in Kelvin.

We have the following information:

n = 0.133 moles (133 mmol of BF3), P = 1 atm (room pressure), R = 0.0821 L·atm/mol·K (this is the value of the ideal gas constant for these units), T = 11.0°C.

The temperature in Kelvin is T(K) = T(°C) + 273.15, so the temperature in Kelvin for this problem is:

T(K) = 11.0°C + 273.15 T(K) = 284.15 K.

Now we can solve for V:

PV = nRT V = nRT / P V = (0.133 mol)(0.0821 L·atm/mol·K)(284.15 K) / (1 atm) V ≈ 3.074 L.

Rounding this to three significant digits, the volume of the boron trifluoride gas collected is approximately 3.07 L.