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because half life will always taking the form of k1/2 = 1/k[A]o (for a zero order reaction) since k is always on the bottom/denominator for any order if it increases then the value of k1/2 (half life) decreases and vice versa
This is because k is associated with how fast a reaction runs. If the reaction runs faster then the amount of time needed for the substance to fall to half its original decreases. Hence, K is inversely proportional to Half life.
amogha_koka3I wrote:Will we be required to know how to derive half-life equations for each order of reaction
I believe this is on the syllabus, and was gone over in lecture so I feel that we are responsible for knowing how to do this.
Half life and k are related differently upon what order the reaction proceeds in. The most common half life problems use first order reactions and this is simply .693/k=t1/2. Therefore you can see the inverse relationship that exists.
Half life is defined as "the time it takes for the concentration of reactant to be half of the original", while k is "the rate at which the reactant is becoming product". The higher k is, the faster the reactant becomes product, the lower the half life will be.
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