The rate constant for a first-order reaction is 3.18 y-1 . If the initial concentration of the reactant is 0.54 M, how many years will it take for the concentration to reach 0.45 M?

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.

The reaction so2cl2(g)→so2(g)+cl2(g) is first order. At 660 k it has a rate contsant of 4.5 X 10^-2 s^-1 Determine the concentration of SO2Cl2 at 15.2 seconds, if the initial concentration is 0.583 M.

At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.00717 s : CICH,CH,CI (g) → CH,CHCI (g) + HCI (g) Suppose a vessel contains CICH,CH,Cl at a concentration of 1.00M. Calculate the concentration of CICH,CH,Cl in the vessel 89.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. |M Ox10 ?

The half-life of a first-order reaction is found to be 28.25 min.What is the value of the rate constant for this reaction?If a 1.00 g sample of reactant is used, what mass will remain after 45 minutes?

Nitrosyl bromide decomposes by the reaction 2 NOBr(g) → 2 NO(g) + Br₂(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. A zero-order reaction is linear when [NOBr] on the y-axis. A first-order reaction is linear when In [NOBr] is on the y-axis. A second-order reaction is linear when 1/[NOBr] is on the y-axis. t [NOBr] 0 0.0653 OM-2.5-2 O M-¹. S-1 What are the units for the rate law? O M-2. s-1 OM-3. s-1 5 15 50 10 85 0.0514 0.0424 0.0361 0.0177 0.0117 What is the rate law for the reaction? (Rate equations take the general form 'rate = k. [A] . [B]'.) What is the value of the rate constant at the temperature of the experiment? 4.0✔ S M chemPad XX⁰ ← → Help Greek

The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 613 K.

The initial concentration of a reactant in a first order reaction is 0.860 M. What will be its concentration after 4 half-lives have passed?

The decomposition of ethylene oxide (CH₂)2O(g) → CH4(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 631 K.

What is the rate constant of a first-order reaction that takes 375 seconds for the reactant concentration to drop to half of its initial value?