Sulfur dioxide is used to make sulfuric acid. One method of producing it is by roasting mineral sulfides, for example,

FeS2(s) + O2(g) —> SO2(g) + Fe2O3(s) (unbalanced)

A production error leads to the sulfide being placed in a 950-L vessel with insufficient oxygen. Initially, the partial pressure of O2 is 0.64 atm, and the total pressure is 1.05 atm, with the balance due to N2. The reaction is run until 85% of the O2 is consumed, andthe vessel is then cooled to its initial temperature. What is the totalpressure and the partial pressure of each gas in the vessel?