Answer:
0.128 atm
Explanation:
There is some info missing. I think this is the original question.
<em>A reaction between liquid reactants takes place at -11.0 °C in a sealed, evacuated vessel with a measured volume of 45.0 L. Measurements show that the reaction produced 35.0 g of chlorine pentafluoride gas. Calculate the pressure of chlorine pentafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 3 significant digits.</em>
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Step 1: Calculate the moles corresponding to 35.0 g of chlorine pentafluoride gas
The molar mass of chlorine pentafluoride gas is 130.44 g/mol. The moles corresponding to 35.0 g of chlorine pentafluoride gas are:

Step 2: Convert the temperature to Kelvin
We will use the following expression.
K = °C + 273.15
K = -11.0°C + 273.15
K = 262.2 K
Step 3: Calculate the pressure of chlorine pentafluoride gas in the reaction vessel after the reaction
We will use the ideal gas equation.
