Do reactions have to have the reversible arrows (one pointing to products and one pointing to reactants) to be a reaction that reaches equilibrium w/forward and backwards movement between products and reactants? It seems EK 1001 Qs for chem describes equations as reaching equilibrium even without reversible arrows but that's different from what I learned.
When finding the equilibrium constant k for a reaction, can we use the coefficients of the molecules involved as the exponents for our equation of products over reactants? Or can we only use the coefficients as exponents for reactions we know to be elementary? EK 1001 doesn't say it's elementary but the answer used coefficients as exponents. How do I know a reaction is elementary without the question specifying it?
Rates of a reaction always increase with temperature. However, if it is a exothermic reaction wouldn't Le Chatelier's say that the rate would decrease if we address the heat as a product? If not the rate directly, the yield of the product decreases, so k decreases, and the rate decreases...or does k stay constant regardless of initial concentration? I wasn't sure what would happen.