2H2(g) + O2(g) = 2H2O(8) If I initially start with 17.00 g of H2 (8) and 37.00 g of O2(e), an analysis of the sample later shows that there are 40.72 g H2O(g) at equilibrium when the reaction is run at 400 K in a 1L container. (a) Find the equilibrium constant for this reaction using pressure (in atmospheres) for the concentration units. (b) What is AG for this reaction? You may assume all gasses behave ideally. Please show all your work