How to set up the rate expressions for the following mechanism? A → B k1
B → A k2
B+C → D k3

If the concentration of B is small compared with the concentrations of A, C, and D, the steady-state approximation may be used to derive the rate law. Derive the rate law, and show that this reaction may follow the first-order equation at high pressures and the second-order equation at low pressures.

Explanation:

From the given information:

A → B k₁

B → A k₂

B + C → D k₃

The rate law =

Using steady-state approximation;

From equation (1), we have:

when the pressure is high;

k₂ << k₃[C]

k₂ >> k₃[C]

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.

hloride, what is the mass of calcium in

explanation: