The reaction A +B+C is found to be zero-order. If it takes 430 seconds for a concentration of A to go from 0.50 M (initial value) to 0.170 M, what is the rate constant for the reaction? Rate constant = M/s

The reaction A + 2B → products was found to be first-order to A and second- order to B. Predict by what factor will the rate of reaction increase when the concentration of A and B are increased to 2 times of the original values at the same time? Please report an integer, without units.

For the reaction 2A + B2→ 2AB, the following information was obtained: Trial [A](M) [B](M) Initial Rate (M/s) 1 1.5 2.0 0.183 2 4.0 3.0 1.098 3 3.0 4.5 1.863 4 1.5 4.0 0.732 5 4.5 2.0 0.549 Determine the rate law and calculate the value of the rate constant. You must justify your answers.

5. You studied the chemical reaction, 2NO2(g) → 2NO(g) + O2(g), at 25°C by monitoring the concentration of NO2(g) as a function of time and constructed the following graph. y= 0.5408x + 125.0 R2=0.998 Time (s) What is the rate constant for this reaction at 25°C? Include the proper units. (W/T) [(3)ONI/T

Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.310 0.230 0.0240 A + B → C + D 2 0.310 0.506 0.116 > 3 0.527 0.230 0.0408 Units k =

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.0066 s 2HI (g) → H, (g) + 12 (g): Suppose a vessel contains HI at a concentration of 0.220M. Calculate how long it takes for the concentration of HI to decrease to 6.0% of its initial may assume no other reaction is important. Round your answer to 2 significant digits.

A particular reaction is found to be zero order. The reactant has an initial concentration of 1.52 M and a rate constant of 0.00740 M/s. Calculate the half life of this reactant in seconds. t1/2 =[A]i/2k

Given the following data, determine the rate constant of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) Experiment [NO] (M) |Ck] (M) Rate (M/s) 0.0300 0.0100 3.4 x 104 0.0150 0.0100 8.5 x 10-5 3 0.0150 0.0400 3.4 x 104

A chemical reaction of the general type:   A → 2B is first-order, with a rate constant of 1.52 × 10-4 s-1. a) Calculate the half-life of A. b) Assuming the initial concentration of A is 0.067 mol L-1, calculate the time needed for the concentration to fall to 0.010 mol L-1.

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