Chapter 12

Question 1

define reaction rate

Answer 1

concentration change/time

Question 2

What is the rate law for this equation :2Na+ O2= 2NaO

Answer 2

Rate=K[Na]^m[O2]^m

Question 3

What is the only way to determine full rate laws?

Answer 3

By looking at experimental data

Question 4

What are the units of K in a first order reaction?

Answer 4

s-1

Question 5

what are the units of K in a second order reaction?

Answer 5

M-1*S-1

Question 6

What is the integrated rate law?

Answer 6

ln [At]/[A0]=-kt

Question 7

If you plot the integrated rate law and the line is straight what order is the reaction?

Answer 7

first

Question 8

What would the slope of a straight integrated rate law be equal to?

Answer 8

-k

Question 9

what is the equation to calculate a first order half life?

Answer 9

t=.693/k

Question 10

What is the integrated rate law for a second order reaction?

Answer 10

1/[At]=kt+1/[A0]

Question 11

In second order reactions is half life dependent upon concentration, and what is the equation?

Answer 11

yes, t1/2=1/k[A0]

Question 12

What is the slope of a integrated second order line equal to?

Answer 12

k

Question 13

What is the difference between an elementary reaction, and a overall reaction?

Answer 13

Elementary is on molecular event, overall is the sum of the elementary steps

Question 14

What is the name of a species that is created in one step, and consumed in the next step?

Answer 14

Intermediate

Question 15

What is the rate law of an elementary reaction?

Answer 15

rate=k[reactants]

Question 16

What step in an overall reaction determines the rate law?

Answer 16

The slow step

Question 17

What is the arrhenius equation?

Answer 17

lnk=(-ea/R)(1/T)+lnA

Question 18

What is the arrhenius equation used for?

Answer 18

calculating activation energy if the rate constant, and temperatures are known.

Question 19

What is a homogeneous catalyst?

Answer 19

A catalyst that is present in the same matter state as the reactants.