🤓 Based on our data, we think this question is relevant for Professor Arasasingham's class at UCI.
For each of the following cases, identify the order with respect to the reactant, A.
Case (A → products) Order
i) The half-life of A is independent of the initial concentration of [A].
ii) A two fold increase in the initial concentration of A leads to a four fold increase in the initial rate.
iii) A two fold increase in the initial concentration of A leads to a 1.41-fold increase in the initial rate.
iv) The time required for [A] to decrease from [A]0 to [A]0/2 is equal to the time required for [A] to decrease from [A]0/2 to [A]0/4.
v) The rate of decrease of [A] is a constant.
i) t1/2=ln2/k This is the only half life equation which is not dependent on the initial concentration of a reactant, and it corresponds to 1st order reaction.
ii) Rate = k[A]x where x is the rate of [A] and overall reaction.
If we increase [A] by 2, the only way for rate to increase by 4 would be if rate or x= 2.
Before: Rate = k2
After: (Rate)4 = k2= k
So this would be 2nd order reaction
iii) Rate = k[A]x