Consider the following reaction: O₂(g) + 2 NO(g) 2 NO₂(g) (a) The rate law for this reaction is first order in O₂(g) and second order in NO(g). What is the rate law for this reaction?

Rate = k [O₂(g)] [NO(g)]

Rate = k [O₂(g)]² [NO(g)]

Rate = k [O₂(g)] [NO(g)]²

Rate = k [O₂(g)]² [NO(g)]²

Rate = k [O₂(g)] [NO(g)]³

Rate = k [O₂(g)]⁴ [NO(g)] (b) If the rate constant for this reaction at a certain temperature is 11900, what is the reaction rate when [O₂(g)] = 0.0218M and [NO(g)] = 0.0297 M? Rate = M/s. (c) What is the reaction rate when the concentration of O₂(g) is doubled, to 0.0436 M while the concentration of NO(g) is 0.0297 M? Rate = M/s