The rate constant for this zero‑order reaction is 0.0240 M ⋅ s − 1 0.0240 M·s−1 at 300 ∘ C. 300 ∘C. A ⟶ products A⟶products How long (in seconds) would it take for the concentration of A A to decrease from 0.900 M 0.900 M to 0.210 M?

It will take for the concentration of A to decrease from 0.900 M to 0.210 M is 28.75 s

Explanation:

Zero order reaction : A reaction is said to be of zero order if the rate is independent of the concentration of the reactants, that means the rate is directly proportional to the zeroth power of the concentration of the reactants.

Expression for the zero order kinetics:

where [A] = concentration left after time t = 0.210 M

= initial concentration = 0.900 M

k= rate constant =

t = time for reaction = ?

Thus it will take for the concentration of A to decrease from 0.900 M to 0.210 M is 28.75 s

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.