QUESTION 1 For the following reaction at 1000 K, 1.04 mol SO2 and 1.12 mol O₂ are placed into a 0.94 L flask. At equilibrium, 0.801 mol of SO3 has been formed. Calculate Kc. Report your answer to the tenths place. 2 SO2(g) + O2(g) = 2 SO3(9) 1.04 1.106 X 8.7 K₁= 0.94 [0.801]² [0.305][0.190] 112 S 01 50₂ 11.106 Ог 1.191 503 0 0.801 -D HDDS +0.801 C 0.801 0.801 x 1/2 50₂ = D.801x1020.4005 773

Suppose a 250. mL flask is filled with 0.40 mol of H₂ and 1.3 mol of HI. This reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of H₂. You can leave out the M symbol for molarity. initial cha equilibrium H₂ 0 X 0 1₂ 0 HI 00 믐 X olo 18 Ar

"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this reaction is one of the ways hydrogen is made industrially. A chemical engineer studying this reaction fills a 500. mL flask with 0.82 atm of carbon monoxide gas and 0.85 atm of water vapor. When the mixture has come to equilibrium she determines that it contains 0.33 atm of carbon monoxide gas, 0.36 atm of water vapor and 0.49 atm of hydrogen gas. The engineer then adds another 0.41 atm of carbon monoxide, and allows the mixture to come to equilibrium again. Calculate the pressure of carbon dioxide after equilibrium is reached the second time. Round your answer to 2 significant digits. atm

I am confused because I am getting two possible answers one being 10. 6 and the other being 1.38