A reaction between liquid reactants takes place at 11.0°C in a sealed, evacuated vessel with a measured volume of 20.0L. Measurements show that the reaction produced 5.0g of sulfur tetrafluoride gas. Calculate the pressure of sulfur tetrafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits.

The pressure of the sulfur tetrafluoride gas is 0.0536 atm

Explanation:

Step 1: Data given

mass of SF4 = 5.0 grams

Molar mass of SF4 = 108.07 g/mol

Temperature = 11.0°C = 273+11 = 284 Kelvin

volume = 20.0 L

Gas constant = 0.08206 L*atm/K * mol

Step 2: Calculate number of moles SF4

Number of moles = mass of SF4 / Molar mass of SF4

Number of moles = 5.0g / 108.07 g/mol = 0.046 moles

Step 3: Calculate pressure via the Ideal gas law

P*V = n*R*T

P = (n*R*T) / V

P = 0.046 * 0.08206 * 284) / 20 = 0.0536 atm

The pressure of the sulfur tetrafluoride gas is 0.0536 atm