CHM 116 Quiz \#3 The following is a proposed reaction to convert a "mixed valency" iron ore to pure iron(III) oxide using nitrogen monoxide: 2Fe3O4(s)+2NO(g)+3Fe2O3(s)+N2O(g) 1) The reaction is to be carried out in a high-temperature reactor having a volume of 2.00L. Calculate G and Kr for this reaction at a temperature of 1250.K. (6 pts) (For Fe3O4(s),H4=1120.9kJmole1 and S=145.5JK1 mole 1 ) 2) 20.000g of the mixed valency iron ore is placed in the reactor, then a vacuum pump is used to evacuate all of the atmospheric gas inside it and decrease the pressure below 104atm. Next, the temperature is raised to 1250 . K, then NO gas is leaked into the reactor from a small, pressurized container called a lecture bottle. If the initial mass of the lecture bottle is 943.27g and its mass decreases to 941.81g after the NO has leaked out of it into the reactor, calculate the partial pressures of the gas-phase species in the reactor, after equilibrium has been achieved. (18 pts) 3) After equilibrium is achieved, the vacuum pump is again used to evacuate the gas in the reactor, then it is cooled back to room temperature and the solid species removed. Calculate the mass of pure Fe2O3 that would be generated in this reaction. (6pts)