The first-order reaction A B has k = 1.25 s, If [Alo 0.450 M, how long...
A first order reaction, where (Alo = 1.00 M, is 69.9 % complete in 383 s. How long does it take for the same reaction to go from 1.00 M to 90.5% completion? Submit Answer Tries 0/45
A zero-order reaction A - B, has a rate constant of 0.725 M. s 1. How long will it take for the concentration of A to decrease from 2.00 M to 1.25 M? 0.967 s 1.03 s 0.750 s 0.725 s 0.103 s
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...
A first order reaction has t1/2 = 13.0 s. How long, in s, does it take for the reactant concentration to decrease to 1.30 % of its initial value ? A. 26 B. 66 C. 39 D. 81 E. 53
A first-order reaction has a half-life of 20.8 s . How long does it take for the concentration of the reactant in the reaction to fall to one-fourth of its initial value?
The rate constant for this first-order reaction is 0.610 s–1 at 400 °C. A--->products How long (in seconds) would it take for the concentration of A to decrease from 0.690 M to 0.260 M? The rate constant for this second-order reaction is 0.590 M–1·s–1 at 300 °C. How long (in seconds) would it take for the concentration of A to decrease from 0.950 M to 0.330 M? The rate constant for this zero-order reaction is 0.0230 M·s–1 at 300 °C...
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...
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 0.693 - 1/2K For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as 1/2 k(Alo Part A A certain first-order reaction (A>products) has a rate constant of 9.60x10 s-1 at45 C. How many minutes does it take for the concentration of the...
Consider the first order reaction, AB2 -> AB + B, which has a first order reaction rate constant of 0.00920 s'. If[AB2] = 0.0100 M at the beginning of the reaction, how many seconds will it take for the concentration to drop to 0.00250 M? a) 151 s b) 75.5 s c) 38.0 s d) 302 s Оа Ob Ос C
If the half-life of a first order reaction is found to be 150 s, how long will it take for the concentration to decrease to 12.5% of the starting concentration for this reaction? 4SOS 150 50 300 Which way will a reaction run if a reaction quotient (Q) is calculated and found to be larger than K for the reaction under the same conditions of temperature and pressure! It will run to the left towards to reactants It will not...