TITLE: REACTION RATE BETWEEN POTASSIUM PERMANGANATE AND OXALIC ACID
EXPERIMENTAL PURPOSE: To determine the rate of a chemical reaction between KMnO4 and H2C2O2 as the concentration are varied
MATERIALS
Aprons
Glasses
Waste bottles
Medium-sized test tubes
250 and 400ML beakers
A white piece of paper
Pipette
Timer
Burette
Erlenmeyer flask
Distilled water
Thermometer
CHEMICALS
KMnO4 (0.130M)
H2C204 (0.755M)
INTRODUCTION
To be in a position to manipulate any operation, one must be aware of every relevant information of the system and how one can use subtle changes to affect the result. If you look at the chemical reaction, it comes from a study of its kinetics where a person gleans the proper understanding to be able to do this. The primary use of chemical kinetics is to measure the speed of chemical reactions. However, most importantly, when measuring the response speed, one gains an understanding of which section of the reaction triggers the speed and therefore allowing the person to suggest a certain way that indicates an analytical reaction. Measuring the chemical reaction speed is the same as measuring speed in general, but instead of discussing the distance traveled by each unit, we measure any who used each time or products produced at another unit. Many factors that affect the chemical reaction are; speed, flexibility, temperature, the surface area of reacting molecules, Catalysts
Concentration molecules must interact with each other to benefit. What is clear from this is that the amount of collision should increase if one increases the number of reactions. This should lead to a faster response rate. Largely in response, this is the case. However, there are many different ways of particular interest in this study is the reaction of potanganum permanganate with oxalic acid. This is the complexity of a diminished response. The interesting part concerning this particular reaction is that potassium permanganate is a purple color but once consumed, it turns a light brown so this reaction can be tested visually. An increase in temperature often increases the rate of a chemical reaction. A close study of this is when making food at home; we normally heat food when we want to eat and freeze the reaming for long-term storage.
EXPERIMENTAL PROCEDURE
While working in pairs, each of the four groups set up three burets, one containing KMnO4, one containing H2C2O4, and one with distilled water. A label was placed on each person for perceiving difficulty with the eyes. The molarities of KMnO4 and H2C2O4 were recorded in Erlenmeyer’s clean and dried flask, the required amount of H2C2O4 was deposited and any water added was washed. Prices set for experiments. The required amount of KMnO4 was placed in a 15cm test tube and permanganate was added to the oxalic acid and the first time the permanganate was released. They were well mixed by swiping the Erlenmeyer flask and the blurring continued until the solution turned a bright yellow / brown color. The time was set and the actual time of the response to the recording occurs.
The second and third tests were repeated and the ratio of these three was considered the response time.
DATA ANALYSIS AND OBSERVATIONS
- Reagent Bottle Concentration of H2C2O4 solution, M:0.755
- Reagent Bottle Concentration of KMnO4 solution, M: 130
- Room temperature, °C:23
When all the reagents were mixed and swirled the color changed from dark purple to a light yellow color and the timer stopped.
| Trial | H2C2O4, mL | KMnO4, mL | DI H2O, mL | Elapsed time, s | ||
| 1 | 20.0 | 10.0 | 0.0 | 215 | ||
| 2 | 20 | 5 | 5 | 250 | ||
| 3 | 10 | 10 | 10 | 420 |
Initial Concentration of KMnO4;
TRIAL #1
M = ()(concentration of KMnO4, M)
Volume of solution = 10
Total volume of mix=30
Concentration of KMnO4 =0.130M
Volume of solution [KMnO4] = Volume of solution (KMnO4) =10 ml X 1 L/1000ml = 0.01L
Total volume of Solution= Vol. of KMnO4 (ml) +Vol. of H2C2O4 (ml) + Vol. of DI H2O (ml)=30 ml
20+10+0=30
So;
#1
M= (10/30)*0.130
=0.043M
#2
M= (5/30)*0.130
=0.022M
#3
M= (10/30)*0.130
=0.043M
Initial H2C2O4 concentration
Initial H2C2O4 concentration, M = ()(concentration of H2C2O4, M)
Volume of solution [H2C2O4] = Volume of solution (H2C2O4) 20ml X 1 L/1000ml = 0.02 L
Total volume of Solution= Vol. of KMnO4 (ml) +Vol. of H2C2O4 (ml) + Vol. of DI H2O(ml)= 30ml
10+20+0=30ml
= Total volume of solution 30 ml X IL/1000ml= 0.03 L
So;
M = ()(concentration of H2C2O4, M)
#1
M=(20/30)*0.775
= 0.52M
#2;
M=(20/30)*0.775
=0.52M
#3
M= (10/30)*0.775
=0.258M
Reaction rate =
#1
Reaction rate= 0.043M/215s
=2.0e-4M/s
#2
Reaction rate=0.022/250
=8.8e-5M/S
#3
Reaction rate= 0.043M/420s
=1.0e-4M/s
Reaction order of H2C2O4,
Rate1 = k [KMnO4]1 x [H2C2O4]1 y Rate1= [KMnO4]1/t1
Rate2 = k [KMnO4]2 x [H2C2O4]2 y Rate2= [KMnO4]2/t2
Rate1/Rate2 = ([KMnO4]1/ [KMnO4]2) x
log10 (ax) = xlog10 (a) (a = [ ])
Experiment #1
2.0*10^-4/1.0*10^-4=0.043*0.52/0.043*0.258
2=2.015
Log2=yLog2.015
y=0.989
1
Experiment #2
2.33=2^x
Log 2.33/log 2= 1.22
Overall reaction order = x + y
= 1+1.22
= 2.22
Rate constant, k
Rate = k[KMnO4]^1.22[H2C204)]^1
2.0e-4M/s=k(0.043)(0.52)
k=0.089M/s
TIME DECREASE =215+250/2
237.5S
237.5/10
=23.75degrees per second
Reaction rate increase
23.75M/s
DISCUSSION AND CONCLUSION
KMnO4 affects the reaction rate more than H2C204 does by speeding it up. The overall order of the reaction for this equation was 2.22.The equation is 0.089M/s[KMnO4]^1.22[H2C204]^1.Water was added to dilute the solution and keep the total volume at 30mL thus slowing down the reaction rate. If not this reaction would have occurred more quickly.
REFERENCES
- Christopher M.Hindson Mechanism of Permanganate Chemiluminescence; Analytical Chemistry 2010;pp4172-4180.
- Militon J.Polissar. The Kinetics of the Reaction between Permanganate and oxalate ions; Physical Chemistry 1935; pp 1057-1066