The reaction shown below is second order and has a rate constant equal to 1.5×107 M-1 s-1 at 0 °C. 2 Mn(CO)5 → Mn2(CO)10 If the initial concentration of Mn(CO)5 is 0.048 M, what is the concentration of the reactant remains after 0.53 s?

The reactant concentration in a second-order reaction was 0.230 M after 230 s and 4.20×10−2 M after 725 s . What is the rate constant for this reaction?

The reaction A → B + C is found to be zero order. If it takes 4.2  102 seconds for an initial concentration of A to go from 0.58 M to 0.29 M, what is the rate constant for the reaction?

Consider the following rate law for the reaction A + B → products. rate = k{A}2{B}2 The reaction is order with respect to A, order with respect to B, and order overall.

It was found that for the reaction 2 A + B → 3 C the rate law is Rate = k[A][B] · %3D At the initial concentrations [A]o = 0.100 M and [B]o = 0.200 M the initial rate is 0.0500 M/s. %3D What would be the initial rate if the initial concentrations were [A]o = 0.500 M and [B]o = 0.0750 M? 0.0352 M/s 0.0937 M/s O 0.0711 M/s 0.00533 M/s O 0.469 M/s

For the following second order reaction, the rate constant is 0.0705.  If [A]0 = 8.22, calculate [A] at 3.16 seconds. 2 A  →  3 B

A reactant decomposes with a half-life of 179 s when its initial concentration is 0.247 M. When the initial concentration is 0.775 M, this same reactant decomposes with the same half-life of 179 s. What is the order of the reaction? 1 2 What is the value and unit of the rate constant for this reaction? k =

The decomposition of nitrous oxide at 565 °C N₂O(g) → N₂ (9)+½O₂(g) 1 is second order in N₂O with a rate constant of 1.10 × 10-³ M s If the initial concentration of N₂O is 2.16 M, the concentration of N₂O will be M after 1480 seconds have passed.

The rate constant for this zero-order reaction is 0.0170 M ·s at 300 °C. A → products How long (in seconds) would it take for the concentration of A to decrease from 0.860 M to 0.320 M? t = S

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