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

Question

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 concentration of reactant after 27.0 hours? 0.0033 M 0.021 M 0.071 M 0.58 M 0.25M Hydrogen peroxide decomposes into water and oxygen in a first-order process. H_2O_2(aq) rightarrow H_2O(I) + 1/2O_2(g) At 20.0degree 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 3.00 days? 0.0033 M 0.0056 M 0.0087 M 0.048 M 0.28M

Explanation / Answer

4) The expression for a first order rate constant is given by,

k1= 2.303/t log (a/a-x) where k1 is rate constant, t is time, a is the initial conc. of reactant, (a-x) is the concentration of reactant after t hrs

Substituting the values, 0.0456 = 2.303/27 log (0.072/ 0.072-x) = 0.085 log

log (0.072/ 0.072-x) = 0.536

(0.072/ 0.072-x) = antilog 3.439

0.072-x= 0.021M

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