The equilibrium constant, kc, for the reaction n2o4 (g) ⇄ 2no2 (g) is 0.211 at 100°c. if the equilibrium concentration of n2o4 is 0.00251 m, calculate the equilibrium concentration of no2. view available hint(s) the equilibrium constant, kc, for the reaction n2o4 (g) ⇄ 2no2 (g) is 0.211 at 100°c. if the equilibrium concentration of n2o4 is 0.00251 m, calculate the equilibrium concentration of no2. 2.65 × 10-4 m 0.0230 m 2.99 × 10-5 m 5.30 × 10-4 m

Achemist at a pharmaceutical company is measuring equilibrium constants for reactions in which drug candidate molecules bind to a protein involved in cancer. the drug molecules bind the protein in a 1: 1 ratio to form a drug-protein complex. the protein concentration in aqueous solution at 25 ˚c is 1.74 x10-6 m . drug a is introduced into the protein solution at an initial concentration of 2.00 x10-6m. drug b is introduced into a separate, identical protein solution at an initial concentration of 2.00 x10-6m. at equilibrium, the drug a-protein solution has an a-protein complex concentration of 1.00 x10-6m, and the drug b solution has a b-protein complex concentration of 1.40 x10-6m.a. calculate the kc value for the a-protein binding reaction.b. calculate the kc value for the b-protein binding reaction.c. assuming that the drug that binds more strongly will be more effective, which drug is the better choice for further research?