A reaction between liquid reactants takes place at −3.0°C in a sealed, evacuated vessel with a measured volume of 5.0L. Measurements show that the reaction produced 17.g 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. Round your answer to 2 significant digits.
Question
A reaction between liquid reactants takes place at −3.0°C in a sealed, evacuated vessel with a measured volume of 5.0L. Measurements show that the reaction produced 17.g 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. Round your answer to 2 significant digits.
Solution
To solve this problem, we need to 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, -3.0°C = -3.0 + 273.15 = 270.15 K.
Step 2: Calculate the number of moles of sulfur tetrafluoride. The molar mass of sulfur tetrafluoride (SF4) is approximately 108 g/mol. So, 17 g of SF4 is 17/108 = 0.157 moles.
Step 3: Substitute the values into the ideal gas law equation. We use the value of R = 0.0821 L·atm/(K·mol) for this calculation. So, P = nRT/V = (0.157 mol * 0.0821 L·atm/(K·mol) * 270.15 K) / 5.0 L = 0.69 atm.
So, the pressure of sulfur tetrafluoride gas in the reaction vessel after the reaction is approximately 0.69 atm.
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