In the reaction: C6H6 + O2 = CO2 + H2O If 26.2 grams of C6H6 is reacted in a 0.250-liter container and this reaction is carried out at 395 K, what is the pressure inside the container?

43.33 atm

Explanation:

We are given;

Mass of C₆H₆ = 26.2 g

Volume of the container = 0.25 L

Temperature = 395 K

We are required to calculate the pressure inside the container;

First, we calculate the number of moles of C₆H₆

Molar mass of C₆H₆ = 78.1118 g/mol.

But; Moles = mass : Molar mass

Moles of C₆H₆ = 26.2 g : 78.1118 g/mol.

= 0.335 moles C₆H₆

Second, we calculate the pressure, using the ideal gas equation;

Using the ideal gas equation, PV = nRT, Where R is the ideal gas constant, 0.082057 L. atm/mol. K

Therefore;

P = nRT : V

= (0.335 mol * 0.082057 * 395 K) : 0.25 L

= 43.433 atm

Therefore, the pressure inside the container is 43.33 atm