Given the standard enthalpy changes for the following two reactions: (1) n2(g) + 2o2(g)n2o4( δh° = 9.2 kj (2) 2n2o(g)2n2(g) + o2(δh° = -164.2 kjwhat is the standard enthalpy change for the reaction: (3) 2n2o(g) + 3o2(g)2n2o4(δh° = ?

Compare the equilibrium constants for the systems shown in the table. which favors products the most? which favors products the least? rank these systems in order from most to least in terms of favoring products rather than reactants. d > b > a > c c > a > b > d b > c > d > a a > d > c > b