Consider two reactions. reaction (1) has a constant half-life, whereas reaction (2) has a half-life that gets longer as the reaction proceeds. what can you conclude about the rate laws of these reactions from these observations? a. the first reaction should have a first or a second order, the second one should have an order greater than second. b.the first reaction is a first order reaction, the second one has a second order. c.the first reaction should have a first or a second order, the second one should have an order not less than second. d.the first reaction is a first order reaction, the second one should have an order greater than first.

Explanation:

1) Reaction 1:

It is stated that reaction 2 has a constant half-life time.

Constant half-life time is a characteristic of first order reactions.

This fact is derived from:

So, the first conclusion is that the first reactions is a first order reaction.

2) Reaction 2.

It is stated that reaction 2 has a half-life that gets longer as the reaction proceeds.

When you do the same analysis for n > 2 (third or higher order reaction), you get the initial concenration raised to a power greater than two in the denominator, driving to the same conclusion, that as the reaction proceeds the half-life gets longer.

So, your second conclusion is that the seond reaction has an order greater than first.

Summarizing the two general conclusions:

That is the choice d. The first reaction is a first order reaction, the second one should have an order greater than first.

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hienas tends to steal pray from other animals. crows and vultures tend to eat dead animals and leftovers.

hope it ,

bioteacher101