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3. A substance reacts according to a second-order rate law. When the initial concentration of the...
The half-life for the second-order decomposition of HI is 15.4 5 when the initial concentration of His 0.67 M. What is the rate constant for this reaction? TT T Arial V3 (12pt) T-E- E- 225
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 4. Cyano...
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A]=[A]0e−kt Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial value. Then we could substitute [A]02 for [A] and rearrange the equation to: t1/2=0.693k This equation calculates the time...
A first order rate law has a rate constant of 0.0011 s-1. If the initial concentration is 4 M. How much is left after 9 minutes?
The integrated rate law allow chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A] = [A]oe -Rt Now say we are particularly interested in the time it would take for the concentration to become one-half of its initial value. Then we could substitute Z" for [A] and rearrange the equation to: A) 1/2= 0093...
At a particular temperature, N2O5 decomposes according to a first-order rate law with a half-life of 3.0 s. If the initial concentration of N2O5 is 1.0 × 1016 molecules/cm3, what will be the concentration in molecules/cm3 after 11.5 s? A. 7.0 × 1014 B. 3.4 × 101 C. 1.0 × 1016 D. 2.0 × 1014 E.
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?
A reactant decomposes with a half-life of 11.5 s when its initial concentration is 0.150 M. When the initial concentration is 0.875 M, this same reactant decomposes with a half-life of 67.1 s. What is the order of this reaction? What is the value and unit of the rate constant for this reaction?
The decomposition of XY is second order in XYand has a rate constant of 7.12×10−3 M−1⋅s−1 at a certain temperature. What is the half-life for this reaction at an initial concentration of 0.100 M? How long will it take for the concentration of XY to decrease to 12.5% of its initial concentration when the initial concentration is 0.100 M? How long will it take for the concentration of XY to decrease to 12.5% of its initial concentration when the initial...
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?