The first order reaction of N2O4 to form two mole of NO2 has a rate constant...
The first order reaction of N2O4 to form two mole of NO2 has a rate constant k = 0.023 min–1. How long will it take the initial concentration of N2O4 to decrease to 10 % of the original value? A. 600s B. 43.5s C. 43.5min D. 435 min E. 100 min
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The first order reaction of N2O4 to form two mole of NO2 has a
rate constant...
The rate constant for the second order reaction 2 NO2 ⟶ N2O4 is 2.79 M-1.min-1 at...
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?
1. A certain first order reaction has a rate constant of 0.036 min-1. How much of the reactant will remain if the reacti...
1. A certain first order reaction has a rate constant of 0.036 min-1. How much of the reactant will remain if the reaction is run for 2.5 hours and the initial concentration of the reactant is 0.31 M? 2. A certain first order reaction has a rate constant of 0.036 min-1. How much of the reactant will remain if the reaction is run for 2.5 hours and the initial concentration of the reactant is 0.31 M? 3. The rate constant...
What are the units of the rate constant for the following reaction? N2O4(g) ---> 2 NO2(g)...
What are the units of the rate constant for the following reaction? N2O4(g) ---> 2 NO2(g) rate = k(N2O4) Can someone please break this down step by step?
A certain reactant disappears by a first order reaction that has a rate constant K= 3.5x10^-3...
A
certain reactant disappears by a first order reaction that has a
rate constant K= 3.5x10^-3 s-1. If the initial concentration of the
reactant is 0.500 M , how long will it take for the concentration
to drop to
0.200 M ?
4. A certain reactant disappears by a first-order reaction that has a rate constant k=3.5 x 10 s. If the initial concentration of the reactant is 0.500 M, how long will it take for the concentration to drop...
5. A student is asked to find the rate constant for a first-order reaction, given that...
5. A student is asked to find the rate constant for a first-order reaction, given that (Alo = 10 M and after 20 s the concentration of A is 2.5 M. The student uses the following logic:2 rate = k[A] (for a first-order reaction) So: A[A] – k[A] Δt' Inserting the values gives: (2.5 M - 10 M - 205-05") = k[2.5 M] Solving for k gives 0.15 5-1. a. Do you agree with the student's answer? Why or why...
The reaction CH, +2C,H, is first order with rate constant k = 1.89 x 10151. a....
The reaction CH, +2C,H, is first order with rate constant k = 1.89 x 10151. a. Suppose that (C.HsJo = 0.265 M. How long (in seconds) will it take for the concentration of CoHs to decrease to 45.0% of its initial value? b. What is the concentration of the product CzHe after 1.75 seconds of reaction?
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate...
2. Answer the following questions by connecting the half-life of each first-order reaction to the rate constant. a. The rate constant of a first-order reaction is 2.43 × 10–2 min–1. What is the half-life of the reaction? (2 points) b. A first-order reaction has a rate constant of 0.547 min-1. How long will it take a reactant concentration 0.14 M to decrease to 0.07 M? (2 points) c. The half-life of a first-order reaction is 5.47 min. What is the...
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order...
1) Hydrogen peroxide, H2O2(aq), decomposes to H2O(l) and O2(g) in a reaction that is first order in H2O2 and has a rate constant k = 1.06×10−3 min−1 at a given temperature. How long will it take for 15% of a sample of H2O2 to decompose? 2)The decomposition of nitrogen dioxide, NO2, into nitrogen monoxide and oxygen at a high temperature is second-order in NO2. The rate constant for this reaction is 3.40 L/mol×min. Determine the time needed for the concentration...
The reaction C H → 2C H is first order with rate constant k = 1.89...
The reaction C H → 2C H is first order with rate constant k = 1.89 x 10-1 s-1. 48 24 a. Suppose that [C4H8]0 = 0.265 M. How long (in seconds) will it take for the concentration of C4H8 to decrease to 45.0% of its initial value
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42...
The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.42 * 10 - 4 s - 1 at a certain temperature. a. What is the half-life for this reaction? b. How long will it take for the concentration of SO2Cl2 to decrease to 25% of its initial concentration? c. If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.78 M? d. If the...
A
certain reactant disappears by a first order reaction that has a
rate constant K= 3.5x10^-3 s-1. If the initial concentration of the
reactant is 0.500 M , how long will it take for the concentration
to drop to
0.200 M ?
4. A certain reactant disappears by a first-order reaction that has a rate constant k=3.5 x 10 s. If the initial concentration of the reactant is 0.500 M, how long will it take for the concentration to drop...
5. A student is asked to find the rate constant for a first-order reaction, given that (Alo = 10 M and after 20 s the concentration of A is 2.5 M. The student uses the following logic:2 rate = k[A] (for a first-order reaction) So: A[A] – k[A] Δt' Inserting the values gives: (2.5 M - 10 M - 205-05") = k[2.5 M] Solving for k gives 0.15 5-1. a. Do you agree with the student's answer? Why or why...
The reaction CH, +2C,H, is first order with rate constant k = 1.89 x 10151. a. Suppose that (C.HsJo = 0.265 M. How long (in seconds) will it take for the concentration of CoHs to decrease to 45.0% of its initial value? b. What is the concentration of the product CzHe after 1.75 seconds of reaction?
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