The steam reforming reaction of methane follows this chemical equation: CH4(g)+H2O(g)CO(g)+3H2(g)rH=+191kJ/mol At 298K the reaction lies far to the reactant side with a very small equilibrium constant of 1.101023. To obtain a significant amount of the desired hydrogen gas product, the reaction is operated at very high temperatures. What is the equilibrium constant at 1100K ? (Note: Some of these numbers have been changed from their actual values for the purpose of the exam.) (Unitless. Do not use scientific notation. Just give the answer as a number with no decimal places) Your