At a certain temperature the following reactic have the constants shown: S(s) + O2(8) = SO2(8) K' = 4.2 x 10 2S(s) + 302(g) = 2SO3(8) K" = 9.8 x 10 %3D Calculate the equilibrium constant K. for the follov ing reaction at that temperature: 2SO,(g) + 0:(g) = 2so

5) At 25 °C the equilibrium constant of the reaction is Kel for the respective reactions and N₂(g) +3H₂(g) 2NH₂(g) (reaction 1) 3.5 x 108. What are the values Ke2 and Ke3 of the equilibrium constants = N2(g) +H₂(g) = NH₂(g) H₂(g) NH3(g), (reaction 2) 2NH3(9) N₂(g) + 3 H₂(g) 1 3 (reaction 3)?

The equilibrium concentrate of H2: 0.048 M The equilibrium concentrate of N2: 0.304M

Use the References to access important values if needed for this question. The equilibrium constant in terms of pressures for the reaction C,H;CH,OH(g)=C,H;CHO(g) + H2(g) is K, = 0.558 at 523 K. (a) A pure sample of gaseous benzyl alcohol, C,H¿CH,OH(g), is introduced into a rigid flask at a temperature of 523 K so that its original pressure is 0.132 atm. Calculate the fraction of this starting material that is converted to products at equilibrium. (b) A second sample of benzyl alcohol is introduced into a rigid flask at a temperature of 523 K, this time at an original pressure of 4.14 atm. Again, calculate the fraction of the starting material that is converted to products at equilibrium.