The rate constant for this zero‑order reaction is 0.0310 M⋅s-1 at 300 ∘C. A⟶products How long (in seconds) would it take for the concentration of A to decrease from 0.830 M to 0.240 M?

A certain first order reaction has k = 2.51 s-1 .  If the initial concentration of the reactant is 6.50 M, how much will be left after two half lives (in M)? Give your answer to three sig figs

The reaction A(aq) → B(aq) is a reaction of order one with respect to A(aq). Theconcentration of A(aq) after 100.0 s of reaction is 0.477 M. The concentration of A(aq) afteranother 300.0 s (so 400.0 s in total) is 0.277 M. What was the initial concentration ofA(aq)? The temperature is always 25.0◦C

The rate constant for this first‑order reaction is 0.0240 s−1 at 400 ∘C. A⟶products After how many seconds will 21.7% of the reactant remain? t=

The rate constant for this second‑order reaction is 0.640 M−1⋅s−1 at 300 ∘C. A⟶products How long, in seconds, would it take for the concentration of A to decrease from 0.820 M to 0.220 M?

The rate constant for the reaction is 0.450 M−1⋅s−1 at 200 ∘C.   A⟶products If the initial concentration of A is 0.00610 M, what will be the concentration after 405 s?

The rate constant for this second-order reaction is 0.780 M-1 ·s-1 at 300 °C. A products How long, in seconds, would it take for the concentration of A to decrease from 0.800 M to 0.390 M?

The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.227 M. What is the value of k for this reaction?

A reaction is found to be first-order with a rate constant of 0.0525 s–1. If the reaction initially began with 5.25 M reactant, how long (in s to the nearest whole number) will it take for 0.20 M reactant to be consumed?

Consider the following reaction. aA +bB →→ cC whose first and second half-lives are 15.9 and 15.9 minutes respectively.  If the rate constant is equal to 0.04358 and [A]0 = 11.98,  calculate the [A] at t = 30.83 minutes.