Given the reaction A+B rightarrow C + D and using delta G degree= -RTIn(K_eq). (Useful calculations: In1=0, ln1=positive.) If the products concentrations equaled 1M and the reactants concentrations equaled 2M at equilibrium, would Delta G degree be positive or negative and would this reaction be favorable or unfavorable as written? If the reaction were favorable, would it be rapid or slow based on the information given? Why or why not? Given that Delta G_relation = Delta G degree + RTIn (Q) and using the jumping bean analogy or puff ball analogy, describe the role of K_eq and Q in determining if a reaction is spontaneous as written. Many reactions that a cell must have occur to live and grow are intrinsically thermodynamically unfavorable (Delta G degree > 0). What is meant by thermodynamically unfavorable how do cells manipulate conditions to allow these reactions to occur?