In an experiment, a 1.5 L flask at 298 K is filled with 1.00 mole of A2 (a diatomic gas) and 1.00 mole of B2 (another diatomic gas). The A2 and B2 react to form AB3. The reaction goes to completion and all gases are ideal. The final total pressure in the flask is found to be 1.25 atm. What is the final composition of the mixture in terms of partial pressures? 

(A) 0.625 atm of A2, 0.625 atm of B2, and 0.625 atm of AB3 

(B) 0.75 atm of A2, 0.5 atm of B2, and 1.25 atm of AB3 

(C) 1.0 atm of A2, 0.25 atm of B2, and 0.75 atm of AB3

(D) 0 atm of A2, 0 atm of B2, and 1.25 atm of AB3

Answer rating: 100% (QA)

The detailed answer for the above question is provided below To find the final composition of the mi... View the full answer