A certain zero order reaction has a half live of 2.5 seconds when the initial concentration...

A certain zero order reaction has a half live of 2.5 seconds when the initial concentration is 2.5 M. What concentration of the reactant remains after 4.5 seconds?
The reaction shown below obeys second order kinetics with k = 2.50 x 10-3 M-1s-1 at 25 oC. If the initial concentration of A is 2.00 M, how long will it take for concentration of A to decrease to 35.0 % of its original value?

A + A → products
For a certain second order reaction, k = 0.075 M‒1s‒1. If 0.0025 M of reactant remains after 15 minutes, how much of the reactant was present initially?
A certain reaction is known to be second order in [A]. What is the numerical value of k, the specific rate constant, if the concentration of [A] decreases from 1.50 M to 0.25 M after 225 seconds?
A certain reaction is known to be second order in A with k = 0.95 M‒1s‒1. What is the numerical value of the half-life (τ1⁄2) when the initial concentration of A is 0.45 M?

Expert Solution

queen_honey_blossom answered 1 year ago

A zero order reaction starts with an initial concentration of reactant of 1.00 M and has...

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Suppose a chemical reaction is first order and has a half-life of 2.5 hr at 100...

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