CH 117 Fall 2015Worksheet 1
1. Define rate as it pertains to a chemical reaction.
2. Consider the following chemical reaction: Mg + 2 H2O ® Mg(OH)2 + H2
a. Write a few rules that govern the rates of appearance and disappearance for each species.
b. If H2O is being consumed at a rate of -0.250 M/s, what is the rate of H2 production?
3. Describe the general rate law expression.
4. A +B ® C
When the reaction given above takes place, the rate law is: Rate = k[A]
If the temperature of the reaction chamber were increased, what will happen to the rate of reaction?
5. If the overall order of a reaction is 0, what are the units of k? Overall order of 1? 2? 3?
6. It is found that doubling the amount of A causes the reaction rate to double while doubling the amount of B causes the reaction rate to quadruple. What is the best rate law equation for this reaction?
7. Given the following information, a) write the rate law for the reaction b) calculate the rate constant. C) What is the rate of the reaction when [ClO2] = 8.25 x 10-3 M and [OH-] = 5.35 x 10-2 M?
Trials / [ClO2] / [OH-] / Rate (M/s)1 / 1.25x10-2 / 1.30 x 10¯3 / 2.33 x 10¯4
2 / 2.50 x 10¯2 / 1.30 x 10¯3 / 9.34 x 10¯4
3 / 2.50 x 10¯2 / 2.60 x 10¯3 / 1.87 x 10¯3
8. Determine the a)rate expression b)rate constant c) reaction rate when [A]= 9x10-2 and [B]= 5.3x10-4
Trials / [A] / [B] / Rate (M/s)1 / .6 / .15 / 6.3 x 10¯3
2 / .2 / .6 / 2.8 x 10¯3
3 / .2 / .15 / 7.0 x 10¯4