Consider the following reaction. aA +bB → → cC whose first and second half-lives are 48.3 and 24.15 minutes respectively. If the rate constant is equal to 0.1362 and [A]0 = 13.16, calculate the [A] at t = 5.69 minutes.
Consider the following reaction. aA +bB → → cC whose first and second half-lives are 48.3 and 24.15 minutes respectively. If the rate constant is equal to 0.1362 and [A]0 = 13.16, calculate the [A] at...
Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 48.6 and 97.2 minutes respectively. If the rate constant is equal to 0.001538 and [A]0 = 13.38, calculate the [A] at t = 22.16 minutes.
Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 12.7 and 12.7 minutes respectively. If the rate constant is equal to 0.05457 and [A]0 = 16.37, calculate the [A] at t = 76.27 minutes.
aA + bB -> cC whose first and second half-lives are 49.6 and 49.6 minutes respectively. If the rate constant is equal to 0.01397 and [A]0 = 10.05, calculate the [A] at t = 21.78 minutes.
1. For the following second order reaction, the half-life is 52.4 and the [A]0 = 3.04. Calculate the rate constant. 2 A →→ 3 B 2. Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 20.9 and 20.9 minutes respectively. If the rate constant is equal to 0.03316 and [A]0 = 10.66, calculate the [A] at t = 19.85 minutes.
A.For the following first order reaction, the half-life is 28.3 and the [A]0 = 1.36. Calculate the rate constant.2A -> 3BB.Consider the following reaction. aA + bB -> cCwhose first and second half-lives are 38.2 and 19.1 minutes respectively. If the rate constant is equal to 0.2148 and [A]0 = 16.41, calculate the [A] at t 5.87 minutes.C.A researcher raises the temperature from 46.4 to 66 °C and finds that the rate of the reaction doubles. What was the activation energy (in...
Determine the first half-life of the reaction. Determine the second and third half-lives. aA - bВ Time [A] (S) 0 0.0100 0.0071 8 0.0055 112 0.0045 16 0.0038
For a first-order reaction, the half-life is constant. It depends only on the rate constant k k and not on the reactant concentration. It is expressed as t1/2=0.693k t 1 / 2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t1/2=1k[A]0. A certain first-order reaction (A→products A → p r o d u c t s ) has a rate constant of 9.30×10−3...
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 t 1/2 = 0.693 k For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and so is expressed as t 1/2 = 1 k[A ] 0 Part A A certain first-order reaction ( A→products ) has a rate constant of 9.90×10−3 s −1 at 45 ∘...
For the following second order reaction, the rate constant is 0.324 and the [A]0 = 2.62. Calculate the half-life. 2 A →→ 3 B
The reaction 2A → B is second order with a rate constant of 51.0/M·min at 24°C. (a) Starting with [A]0 = 9.30 × 10−3 M, how long will it take for [A]t = 2.70 × 10−3 M? (b) Calculate the half-life of the reaction. Answer in Minutes