How Fast is the Reaction Happening?

What is the value and unit of the rate constant (k) for this reaction?

When the initial concentration is 0.380 M, this reactant decomposes with a half-life of 129 s. What is the rate constant?

What is the order of the reaction?

Can you determine the order of the reaction based on the given data?

Answer:

A) The rate constant is 0.0078 s^-1

B) The order of the reaction is 1

In the given scenario, the initial concentration of the reactant is 0.380 M, and it decomposes with a half-life of 129 s. When calculating the rate constant (k) and the order of reaction, we find that the rate constant is 0.0078 s^-1 and the order of the reaction is 1.

For the rate constant calculation, we use the formula Rate = k[Reactant]^n. By substituting the initial concentration, half-life, and final concentration, we can determine the rate constant to be 0.0078 s^-1.

Similarly, to find the order of the reaction, we use the relationship between rate and concentration for reactant decomposition. By solving the equation, we can establish that the reaction is first order (n=1).