What advantages or disadvantages do initial rate studies have in comparison to time course studies in determining the order of the reaction with respect to a given reactant

A particular reactant decomposes with a half-life of 129 s when its initial concentration is 0.280 M. The same reactant decomposes with a half-life of 209 s when its initial concentration is 0.173 M. Determine the reaction order. 2 What is the value and units of the rate constant for this reaction? k = Units

The rate of a certain reaction was studied at various temperatures. The table shows temperature (?) and rate constant (?) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, ?a , for this reaction? What is the value of the pre‑exponential factor (sometimes called the frequency factor), ? , for this reaction? Temperature (K)      k (s^-1)    400                           0.0000173 580                            7.43

Suppose that the half-life of a stimulant shot into a race horse is 28 days. Assuming the stimulant biodegrades by a first-order process, how long will it take for 1/32 of the initial dose to remain in the horse’s body?

How can measurements of reaction half-lives be used to determine the order of a reaction?

A particular reactant decomposes with a half-life of 151 s when its initial concentration is 0.289 M. The same reactant decomposes with a half-life of 239 s when its initial concentration is 0.183 M. Determine the reaction order. 1 2 0 What is the value and units of the rate constant for this reaction?

It has been found that DDT in the soil decomposes by a first-order reaction with a half-life of 12.0 years. How long would it take DDT in a soil sample to decompose from a concentration of 165 ppbm (parts per billion by mass) to 15 ppbm?

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?

The half-life of a reaction, t/2. is the time it takes for the reactant concentration A| to decrease by half. For example, after one half-life the concentration falls from the initial concentration [Alo to [Alo/2, after a second half-life to [A]o/4, after a third half-life to [Alo/8. and so on. on.

Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: step elementary reaction 1 NO (g) + Br₂ (g) → NOBr₂ (g) k₁ k₂ 2 NOBr₂ (g) + NO (g) → 2NOBr (g) Suppose also k₁ « k₂ . That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant 010 X Ś