In the first-order reaction A→products, it is found that 99 % of the original amount of reactant A decomposes in 144 min .
A° = 100
A(final) = 100-99 = 1
Time = 144 min
Ln( A°/A ) = rate constant * time
Ln(100/1) = rate constant * 144
Rate constant = 0.032
Half Life = 0.693 / rate constant
= 0.693 / 0.032
= 21.67 min
If you have any questions please comment
If you satisfied with the solution please rate it thanks
In the first-order reaction A→products, it is found that 99 % of the original amount of...
What statement is true? For the first-order reaction, A → products, 12.5% of initial amount of A is left after two half-lives. For the first-order reaction, A → products, if half of the initial concentration of A reacts in 20 min, then the remaining half will completely react in the next 20 min. For the first-order reaction, A → products, 25% of initial amount of A is left after two half-lives. For the first-order reaction, A → products, 75% of...
The reaction, aA products, is a first order reaction with a rate constant of 1.248 x 10-4 s-1 . a. How long (in seconds) does it take for the initial amount of A to decrease by 30%? b. What fraction of reactant remains after 30 minutes? c. What is the half-life for the reaction? d. How long does it take for the initial amount of reactant to decrease by 87.5%?
A certain first-order reaction (A products) has a rate constant of 5.40 10-3 s I at 45 °C How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration? at 27 °C A certain second-order reaction (B-products) has a rate constant of 1.05x10-3 M 1.s and an initial half-life of 266 s What is the concentration of the reactant B after one half-life?
Part A. A certain first-order reaction (A→products) has a rate constant of 3.90×10−3 s−1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration? Part B. A certain second-order reaction (B→products) has a rate constant of 1.90×10−3 M−1⋅s−1 at 27 ∘C and an initial half-life of 298 s . What is the concentration of the reactant B after one half-life?
A certain first-order reaction (A→products) has a rate constant of 5.70×10−3 s−1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration?
A certain first-order reaction (A?products) has a rate constant of 5.70×10?3 s?1 at 45 ?C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration?
A certain first-order reaction ( A products) has a rate constant of 5.10x10-35-1 at 45 °C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25% of the original concentration? Express your answer with the appropriate units. View Available Hint(s) ? HA Value O Units Submit Part B A certain second-order reaction (B>products) has a rate constant of 1.10x10-3M-1.s-1 at 27°C and an initial half-life of 212 s . What is the concentration...
a first order reaction with a single reactant (A) is found to have a half-life of 69.4 seconds. 1) calculate the rate constant for the reaction 2) if [A]0=0.100 M , calculate [A]t at 60.0 seconds 3) how long will it take , in mintues for 90.0 % of A to decompose ?
A certain first-order reaction (A→products) has a rate constant of 1.00×10−2 s-1 at 45 ∘C. How many minutes does it take for the concentration of the reactant, [A], to drop to 6.25%% of the original concentration? Express your answer with the appropriate units.
39. A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C. a. Write a rate law for the reaction. b. What is the overall order of the reaction? c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled (and the...