The rate constant for the second order reaction is 0.200 How long in seconds would it...

Question

Question

The rate constant for the second order reaction is 0.200

How long in seconds would it take for the concentration of A to decrease from 0.830 M to 0.240 M

Answer 1

Answer #1

Second onder roate equation, 1 kt = 1 / - LAS ove, Putting values on abure equation, ozvob Rate constant, K = 0.200. Initial

Answer 2

Similar Homework Help Questions

The rate constant for this first-order reaction is 0.610 s–1 at 400 °C. A--->products How long...

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...
The rate constant for this second-order reaction is 0.400 M-'.5' at 300 °C. A products How long, in seconds, would...

The rate constant for this second-order reaction is 0.400 M-'.5' at 300 °C. A products How long, in seconds, would it take for the concentration of A to decrease from 0.770 M to 0.360 M? R. T U T O P F G H J K L NM <
The rate constant for this second-order reaction is 0.460 M–1·s–1 at 300 °C. How long (in...

The rate constant for this second-order reaction is 0.460 M–1·s–1 at 300 °C. How long (in seconds) would it take for the concentration of A to decrease from 0.630 M to 0.340 M?

The rate constant for this second-order reaction is 0.940 M1s-1 at 300 °G A products How...

The rate constant for this second-order reaction is 0.940 M1s-1 at 300 °G A products How long (in seconds) would it take for the concentration of A to decrease from 0.670 M to 0.290 M? Number
The rate constant for this second‑order reaction is 0.300 M−1⋅s−1 at 300 degrees C. A⟶products How...

The rate constant for this second‑order reaction is 0.300 M−1⋅s−1 at 300 degrees C. A⟶products How long, in seconds, would it take for the concentration of A to decrease from 0.630 M to 0.300 M
The rate constant for this second-order reaction is 0.430 M-'.s at 300 °C. A- products How...

The rate constant for this second-order reaction is 0.430 M-'.s at 300 °C. A- products How long, in seconds, would it take for the concentration of A to decrease from 0.670 M to 0.310 M? 1 = 6.355 Incorrect Calculate the rate constant, k, for a reaction at 56,0 °C that has an activation energy of 88.6 kJ/mol and a frequency factor of 6.85 x 10's-1 k= 2.2188 SI Incorrect

The rate constant for this zero‑order reaction is 0.0380 M⋅s−1 at 300 ∘C. A⟶products How long...

The rate constant for this zero‑order reaction is 0.0380 M⋅s−1 at 300 ∘C. A⟶products How long (in seconds) would it take for the concentration of A to decrease from 0.890 M to 0.300 M?
The rate constant for this first-order reaction is 0.150 s- at 400 °C. A products How...

The rate constant for this first-order reaction is 0.150 s- at 400 °C. A products How long, in seconds, would it take for the concentration of A to decrease from 0.730 M to 0.260 M? t = S
The rate constant for the second-order reaction: 2N02(g)-→ 2NO(g) + O2(g) is 0.54/M s at 300°C...

The rate constant for the second-order reaction: 2N02(g)-→ 2NO(g) + O2(g) is 0.54/M s at 300°C 2 M to 0.28 Mn (a) How long (in seconds) would it take for the concentration of NO2 to decrease from 0.6 (b) Calculate the half-lives at these two concentrations.

The second-order reaction shown below has a rate constant of o.510 M-1 s1 at 250°0C. A...

The second-order reaction shown below has a rate constant of o.510 M-1 s1 at 250°0C. A → products If you started with o.700 M of A, how long would it take (in seconds) for the concentration to decrease to o.220 M? Consult Textbook Numerical Answer: