Consider the following initial rate data (at 273 K) for the decomposition of a substrate (substrate 1) which decomposes to product 1 and product 2: [Substrate 1] (M) Initial Rate (M/s) 0.4 0.183 0.8 0.183 2 0.183 Determine the half-life for the decomposition of substrate 1 when the initial concentration of the substrate is 2.77 M.

15.1 seconds is the half life of the reaction when concentration of the substrate is 2.77 M.

Explanation:

A → B + C

The rate law of the reaction will be :

Initial rate of the reaction when concentration of the substrate was 0.4 M:

..[1]

Initial rate of the reaction when concentration of the substrate was 0.8 M:

...[2]

[1] ÷ [2] :

x = 0

The order of the reaction is zero.

For the value of rate constant ,k:

..[1]

x = 0

k= 0.183 M/s

The half life of the zero order kinetics is given by :

Where:

= Initial concentration of A

k = Rate constant of the reaction

So, the half-life for the decomposition of substrate 1 when the initial concentration of the substrate is 2.77 M:

15.1 seconds is the half life of the reaction when concentration of the substrate is 2.77 M.

- decrease the number of plants and animals living in the water.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.