rate constant is k = 0.330 M -1
S-1
units of the K indicates that the order is second order
the integrated rate law is as follows
1 / [A] = kt + 1 / [A]0
here the [A] = concentration after time
[A]0 = initial concentration
k = rate constant = 0.330 M-1 s-1
t = time = 895 sec
substituting the values
1 / [A] = kt + 1 / [A]0
1 / [A] = 0.330 * 895 + 1 / 0.00120
1 / [A] = 0.330 * 895 + 833.33
1 / [A] = 1128.68
=> [A] = 0.0008859 M
answer => 0.0008859 M (or) 8.86*10-4 M
- The rate constant for the reaction is 0.330 M-'.-' at 200 °C. A — products...
Atter The rate constant for the reaction is 0.720 M-'.-' at 200 °C. A products If the initial concentration of Ais 0.00760 M, what will be the concentration after 775 s? [A] = .137
The rate constant for the reaction is 0.120 M-!. s-1 at 200 °C. A products If the initial concentration of A is 0.00160 M, what will be the concentration after 245 s? [A] - M
The rate constant for the reaction is 0.510 M-1.5-1 at 200 °C. A products If the initial concentration of A is 0.00120 M, what will be the concentration after 675 s? [A] =
The rate constant for the reaction is 0.340 M-1.5-lat 200 °C. A — products If the initial concentration of A is 0.00260 M, what will be the concentration after 195 s? [A] = 2.6 x104
The rate constant for the reaction is 0.600 m–1·s–1 at 200 °c. If the initial concentration of A is 0.00630 M, what will be the concentration after 455 s?
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...
A certain second-order reaction (B→products) has a rate constant of 1.20×10−3 M−1⋅s−1 at 27 ∘C and an initial half-life of 260 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 5.40 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?
Use the table below to solve for the rate constant for the reaction A + 2B + 2C - products. Trial [A], M 0.420 1 [B],M 0.150 0.150 [C],M Initial rate, M/s 0.330 4.00 0.330 4.00 2 0.210 3 0.420 0.225 0.330 6.00 4 0.420 0.150 0.660 8.00 Type in a numerical answer only with the correct sig figs. Do NOT type in units.
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?