What is the partial pressure (in atm) of CO₂ at 468.2 K in a 25.0 L fuel combustion vessel if it contains 60.0 grams CO₂, 82.1 g H₂O, and 7.30 mol vaporized, yet uncombusted fuel?

2.09 atm

Explanation:

Step 1: Given and required data

We won't need the data of water and uncombusted fuel, since the partial pressures are independent of each other.

Step 2: Calculate the number of moles (n) corresponding to 60.0 g of CO₂

The molar mass of CO₂ is 44.01 g/mol.

60.0 g × 1 mol/44.01 g = 1.36 mol

Step 3: Calculate the partial pressure of CO₂

We will use the ideal gas equation.

P × V = n × R × T

P = n × R × T/ V

P = 1.36 mol × (0.0821 atm.L/mol.K) × 468.2 K/ 25.0 L = 2.09 atm

b is the correct answer

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