Chemical Equilibrium and Kinetics
Discussion Our experiment is divided into 9 parts:
A. Effect of Nature of Reactants to the reaction rate.
B. Effect of Temperature to the reaction
C. Effect of Concentration to the Reaction Rate
D. Effect of Catalyst to the Reaction Rate
E. Chromate-Dichromate Equilibrium
F. Thiocyanatoiron (III) Complex Ion Equilibrium
G. Weak Acid Equilibrium (Ionization of Acetic Acid)
H. Weak Base Equilibrium Ionization of Ammonia
I. Saturated Salt (Sodium Chloride) Equilibrium
On part (A) we are to observe which reaction rate is faster, and doing the experiment. We have concluded that:
“Aluminum had faster rate of reaction rate than iron because it is more active than iron based on the activity series.”
TABLE B.
Temperature (C)
Time to complete the reaction
30’C
22 seconds
50’C
20 seconds
70’C
18seconds
In this part, we have concluded that as temperature increases, the reaction rate increases also.
TABLE C.
HCL concentration
Time to complete the reaction
0.5M
134 seconds
1.0M
79 seconds
1.5M
59 seconds
In this part, we have concluded that as concentration increases, the reaction rate also increases.
Part (D) “The effect of cupric sulfate solution enhanced the rate of decomposition of hydrogen peroxide.”
Chemical equilibrium is the state of constant composition attained when opposing reaction rates become equal. There is an essential relationship between reaction rates and chemical equilibrium, one that we can describe quantitatively. At first thought, the connection may seem obscure - do we not need to be far from equilibrium to properly measure reaction rates? The dynamic nature of chemical equilibrium means that both forward and reverse reactions can be taking place at significant - even high - rates, but since these rates are equal, no change in concentration is observed over time.
Let us once again use the hypothetical example of a simple, reversible reaction, A = B (such as an isomerization) to show the approach to
A. Effect of Nature of Reactants to the reaction rate.
B. Effect of Temperature to the reaction
C. Effect of Concentration to the Reaction Rate
D. Effect of Catalyst to the Reaction Rate
E. Chromate-Dichromate Equilibrium
F. Thiocyanatoiron (III) Complex Ion Equilibrium
G. Weak Acid Equilibrium (Ionization of Acetic Acid)
H. Weak Base Equilibrium Ionization of Ammonia
I. Saturated Salt (Sodium Chloride) Equilibrium
On part (A) we are to observe which reaction rate is faster, and doing the experiment. We have concluded that:
“Aluminum had faster rate of reaction rate than iron because it is more active than iron based on the activity series.”
TABLE B.
Temperature (C)
Time to complete the reaction
30’C
22 seconds
50’C
20 seconds
70’C
18seconds
In this part, we have concluded that as temperature increases, the reaction rate increases also.
TABLE C.
HCL concentration
Time to complete the reaction
0.5M
134 seconds
1.0M
79 seconds
1.5M
59 seconds
In this part, we have concluded that as concentration increases, the reaction rate also increases.
Part (D) “The effect of cupric sulfate solution enhanced the rate of decomposition of hydrogen peroxide.”
Chemical equilibrium is the state of constant composition attained when opposing reaction rates become equal. There is an essential relationship between reaction rates and chemical equilibrium, one that we can describe quantitatively. At first thought, the connection may seem obscure - do we not need to be far from equilibrium to properly measure reaction rates? The dynamic nature of chemical equilibrium means that both forward and reverse reactions can be taking place at significant - even high - rates, but since these rates are equal, no change in concentration is observed over time.
Let us once again use the hypothetical example of a simple, reversible reaction, A = B (such as an isomerization) to show the approach to