A reaction has a rate law of Rate = (1.25 Ms)[A][B]. What concentration of [B] would give the reaction a rate of 0.0421 if the concentration of [A] is 0.250 M?

The reaction A + 2B + C Products has a rate law of Rate = k[A][B]. By what factor would the reaction rate change if [C] is tripled?

How long will it take for the concentration of A to decrease from 1.400 M to 0.265 for the zero order reaction A Products? (k = 0.0345 M/s)