Question

Rate constant?

Some measurements of the Initial rate of a certaln reactlon are glven In the table below. H2initial rate of reaction 1.31 M 0.797 M 3.56 M 0.797 M 1.31 MI 2.16 M 42.0 Mis 114. M/s 114. M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol.

Answer 1

Rate lavw Rate-k[Hal"[12]у k- rate constant x and v= partial orders Calculate x (partial order for H2) 42.0 -k[1.31] [0.797] 114 k[3.56]a [0.797] 42.0 [1.31] [o.797 114 3.56140797)" 42.0 [1.31]x 114 [3.56]х 42.0 1.31 1143.56 0.3684 = (0.3680)" log0.3684 log (0.3680) log0.3684 x log 0.3680 log0.3684 log 0.3680

Calculate y (partial order for I2) 2.0-k[1.31]"[0797]y 114 k[1.31] [2.16] 42.0 [1-3-T[0.797]y 114 kt13t "[2.16]y 42.0 [1.31] 114 [2.16]3 42.0 1.31 114 2.16 0.3684 (0.6065) 4

log0.3684 log (0.6065) log0.3684-y log 0.6065 log0.3684 log 0.606!5 yV Rate law Rate k[H21 212 Rate k[b][12] Calculate the rate constant 42.0-= k [1.31 M] [0.797 M]2 42.0k x 0.832 Ms 42.0 0.832 M3 50 M-2s-1-k|