The rate constant of a first-order decomposition reaction is 0.0456 hrs^-1. If t

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The rate constant of a first-order decomposition reaction is 0.0456 hrs^-1. If the initial concentration of reactant is 0 072 M. what is the concentrate of reactant after 27 0 hours? 0.0033 M 0.021 M 0.071 M 0.58M 0.25M Answer: b Hydrogen peroxide decomposes into water and oxygen in a first-order process. H_2O_2 (aq) rightarrow H_2O (I) + 1/2 O_2 (g) At 20.0 degree C, the half-life for the reaction is 3 92 times 10^4 seconds. If the initial concentration of hydrogen peroxide is 0 32 M. what is the concentration after 3000 days? 0.0033 M 0.0056 M 0.0087 M 0.048 M 0.28M Answer a For the second-order reaction below, the rate constant of the reaction is 3 9 times 10^-5 M^-1 s^-1. How long (in seconds) is required to decrease the concentration of A from 1.07 M to 0.24 M? 2A rightarrow B rate = k[A]^2 5.8 times 10^3 s 6.5 times 10^3 s 2.1 times 10^4 s 3.8 times 10^4 s 8.3 times 10^4 s Answer e Calculate the activation energy, E_a for N_2O_5 (g) rightarrow 2 NO_2(g) + 1/2 O_2(g) given k (at 45.0 degree C) = 5.79 times 10^-4 s^-1 and k (at 60.0 degree C) = 3.83 times 10^-3 s^-1. (R = 8.314 J/K mol) 0.256 kJ/mol 2.83 kJ/mol 31.1 kJ/mol 111 kJ/mol 389 kJ/mol Answer: d The mechanism of a chemical reaction is given below. (CH_3)_3 CCl rightarrow (CH_3)_3C^+ + Cl^- (slow) (CH_3)_3C^+ + OH^+ rightarrow (CH_3)_3 COH (fast) Which of the following statements concerning the reaction is/are CORRECT? The overall balanced reaction is: (CH_3)_3 CCl + OH^- rightarrow (CH_3)_3 COH + Cr Chloride ion is a reaction intermediate. The following rate law is consistent with the mechanism rate = K[(CH_3)_3 CCl].

Explanation / Answer

1. B

2. A

3. Didnt get any answer there

4. D

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