Question

1.

The following chemical reaction: A → products shows first order kinetics with respect to A; rate = k[A].

Assume k = 10.09 x 10^-4 s^-1 .

If the initial concentration of A was 0.82 mol L^-1 and then decreased to 0.11 mol L^-1 , how much time elapsed in minutes?

2.

Consider the following balanced chemical equation:

H₂O_{2 (aq)} + 3 I^-_(aq) + 2 H⁺_(aq) → I₃^- _(aq) + 2 H₂O _(l)

In the first 62.9 seconds of the reaction, the concentration of I₃^- increased from 0.202 M to 1.001 M.

What is the average reaction rate over this time interval (in mol L^-1 s^-1)?

3.

Consider the following balanced chemical reaction:

A + B → C

The following table shows initial reaction rates obtained using different initial concentration of A and B:

Initial [A] (mol L-1)	Initial [B] (mol L-1)	Initial Rate (mol L-1 s-1)
0.134	0.244	0.076
0.269	0.244	0.075
0.134	0.734	0.227
0.269	0.734	0.226

4.

The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A]².

If k = 5.95 x 10^-4 mol^-1 L s^-1 and the initial concentration of A is 1.12 mol L^-1, what is the half life of this reaction in minutes?

5.

The following chemical reaction: A → products shows second order kinetics with respect to A; rate = k[A]².

Assume k = 8.9 x 10^-4 mol^-1 L s^-1 .

If the initial concentration of A was 1.20 mol L^-1 and then decreased to 0.069 mol L^-1 , how much time elapsed in minutes?

6.

The following chemical reaction: A → products shows zero order kinetics with respect to A; rate = k[A]⁰.

If k = 5.99 x 10^-4 mol L^-1 s^-1 and the initial concentration of A is 0.208 mol L^-1, what is the half life of this reaction in minutes?

Answer 1