Question

A reaction between liquid reactants takes place at in a sealed, evacuated vessel with a measured volume of . Measurements show that the reaction produced 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 significant digits.

Answer 1

Answer:

0.128 atm

Explanation:

There is some info missing. I think this is the original question.

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.

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:

$35.0g \times \frac{1mol}{130.44g} = 0.268 mol$

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.

$P \times V = n \times R \times T\\P = \frac{n \times R \times T}{V} = \frac{0.268mol \times \frac{0.0821atm.L}{mol.K} \times 262.2}{45.0L} = 0.128 atm$