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What is the half life for a zero order reaction?

Zero-Order Reactions

Zero-Order First-Order
plot needed for linear fit of rate data [A] vs. t ln[A] vs. t
relationship between slope of linear plot and rate constant k = −slope k = −slope
half-life t1/2=[A]02k t1/2=0.693k
Table 22. Summary of Rate Laws for Zero-, First-, and Second-Order Reactions

What is the half life equation for first order?

The half-life of a reaction is the time required for the reactant concentration to decrease to one-half its initial value. The half-life of a first-order reaction is a constant that is related to the rate constant for the reaction: t1/2 = 0.693/k. Radioactive decay reactions are first-order reactions.

What is a zero order reaction?

Zero order reaction simply means that the rate of reaction is independent of concentration of reactants.

Which of the following represents the equation for a second-order half-life?

Chemical Kinetics

Question Answer
Which of the following represents the equation for a second-order half-life? t 1/2= [A]o/2k
Which of the following represents the equaton for a zero-order half-life? t 1/2= [A]o/2k
Which of the following reactions would you predict to have the smallest orientation factor? NOCl2 + NO –> 2 NOCl

Are second-order reactions faster than first-order?

For two or more reactions of the same order, the reaction with the largest rate constant is the fastest. Because the units of the rate constants for zeroth-, first-, and second-order reactions are different, however, we cannot compare the magnitudes of rate constants for reactions that have different orders.

What is the difference between first and second-order system?

There are two main differences between first- and second-order responses. The first difference is obviously that a second-order response can oscillate, whereas a first- order response cannot. The second difference is the steepness of the slope for the two responses.

What is the rate constant for first-order reaction?

k is the first-order rate constant, which has units of 1/s. The method of determining the order of a reaction is known as the method of initial rates. The overall order of a reaction is the sum of all the exponents of the concentration terms in the rate equation.