1. | The second-order rate constant for self-reaction of hydroxyl
radicals 2 OH → H2O + O has the value 1.0786E9 M-1·s-1 at 360.0 K. Compute the half-life of OH radicals at this temperature if the initial concentration is 6.74E-6 M. |
3. |
Calculate the initial rate of
a first-order reaction if the concentration of reactant is 0.37 M
and the half-life is 4.48 s. Enter the correct numerical value to 2.0% precision. Express scientific notation like 4.29E-15 M·s-1 |
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4. | Cyano radicals abstract H
atoms from methane at 349.0 K according to the second-order
reaction CN + CH4 → HCN + CH3 Under conditions where [CH4] = 0.487 M is present in great excess (i.e. pseudo-first-order conditions), the concentration of [CN] was observed to decrease from 2.604E-6 M to 8.5079E-8 M in 11.5 ns. Calculate the second-order rate constant for the reaction under these conditions. M-1·s-1 |
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5. | Consider the hypothetical
reaction A → products Determine the order of the reaction given the initial reaction rates below.
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6. | Consider the generalized
second-order reaction R → products If the initial concentration is [R]0 = 3.307E-6 M and the half-life is 930.0 microseconds, compute the rate constant for the reaction. M-1·s-1 |
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7. | A sample of ancient linen
cloth weighing 21.0 mg produces 0.132813 14C
disintegration counts per second (cps), compared with 13.88 cps
obtained from a 1.000 g calibration standard of contemporary
organic material. From this measurement, determine the apparent age
of the linen sample. |
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8. | Hydroperoxy radicals undergo
the second-order self-reaction 2 HO2 → H2O2 + O2 The rate constant for this reaction is 7.5621E8 M-1·s-1 at 856.0 K. If the initial concentration of HO2 is 1.67E-6 M, compute the time required for the concentration to be reduced to 0.500E-6 M s |
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9. | Gaseous cyano radicals react
with oxygen according to CN + O2 → OCN + O The rate constant for this reaction at 885.0 K is 8.3456E9 M-1·s-1. If [O2] = 0.15 M and is present in great excess (i.e., pseudo-first-order conditions where [O2]>>[CN]) what is the predicted half-life of cyano radicals under these conditions? s |
1. The second-order rate constant for self-reaction of hydroxyl radicals 2 OH → H2O + O...
Cyano radicals abstract H atoms from methane at 389.0 K according to the second-order reaction CN + CH4 → HCN + CH3 Under conditions where [CH4] = 0.493 M is present in great excess (i.e. pseudo-first-order conditions), the concentration of [CN] was observed to decrease from 1.807E-6 M to 2.0167E-12 M in 34.5 ns. Calculate the second-order rate constant for the reaction under these conditions.
1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units of k for this reaction? If the concentration of air decreases by a factor of 2 and the concentration of b increases by a factor of 5 what happens to the rate? 2. for the forward reaction 2NO+Cl2=>2NOCl. determine the rate(m/s)for experiment #4 given [NO]°(M)=0.40M and [Cl2]°z(M)=0?20M. Rate? 3.The following data were collected over time for the forward reaction 2NO2=>2NO+O2 ( 1/[NO2]=100 at 0...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k k and not on the reactant concentration. It is expressed as t1/2=0.693k t 1 / 2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t1/2=1k[A]0. A certain first-order reaction (A→products A → p r o d u c t s ) has a rate constant of 9.30×10−3...
3. Determine a value of the pseudo-order rate constant, kobs. What is the half-life of the reaction under the conditions of the experiment? For how many half-lives was the reaction allowed to run? C9H8O4 + NaOH -------> C9H7O4Na + H2O Concentration of C9H8O4 = 5x10-4M NaOH = 7.1x10-5M **Second order reaction in respect to acetylsalicylic acid. **The rate law may be written as, rate = k[asp]m[OH– ]n and The pseudo-rate law is rate = kobs[asp]m Where kobs = k[OH– ]n...
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant concentration. It is expressed as t 1/2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t 1/2 = 1 k[A ] 0 Part A A certain first-order reaction ( A→products ) has a rate constant of 9.90×10−3 s −1 at 45 ∘...
The rate constant for the second order reaction 2 NO2 ⟶ N2O4 is 2.79 M-1.min-1 at 48oC. If the initial concentration of NO2 is 1.05 M, what is the half-life?
4) What is the half-life of a second order reaction with the rate constant 0.0271 m 's and the initial concentration 0.902M?
2. Consider the second order reaction 2NOB → 2NO+ Br2 The rate constant is 0.80 M-1 5-1. The initial concentration is 0.86 M. 4) Find the half-life of the reaction. 5) Find the concentration of PH3 after 10 min. 6) How long will it take for the concentration of PH3 deceased to 0.01 M. how transcribed image text
A certain second-order reaction (B→products) has a rate constant of 1.20×10−3 M−1⋅s−1 at 27 ∘C and an initial half-life of 260 s . What is the concentration of the reactant B after one half-life?
2. The reaction A → products was found to be second order order and have a rate constant, k, of 0.681 M-1 5-1. If the initial concentration of the reaction was 0.885 M, what is the half life for the reaction? 10.2 Submit Answer Incorrect. Tries 5/45 Previous Tries