Rate of Reaction Investigation
Aim:
To determine how changing the concentration of a reactant (Na S O )
affects the rate of the reaction.
Prediction:
I predict that when we increase the concentration, the rate will
increase; therefore there are more particles and a greater probability
of a collision. If more particles are present in the same volume, they
will be closer together. This means they have a higher probability of
colliding and speeding up the reaction.
If we double the concentration, the rate will also double.
Text Box: 200ml Beaker of Sodium ThiosulphateText Box: 200ml Beaker of Hydrochloric Acid[IMAGE][IMAGE][IMAGE][IMAGE][IMAGE]Diagram:
[IMAGE][IMAGE]Text Box: Conical Flask
Paper
Timer
Big Measuring Cylinder
Small Measuring
Cylinder
[IMAGE]
Apperatus:
200 ml Beakers – To hold solutions
Lined paper – To determine when the mixture is cloudy
Timer – To time the rate of reaction
Hydrochloric acid
Sodium thiosulphate
Water
100ml measuring cylinder
10ml measuring cylinder
Fair Test:
For a fair test I must do:
· Make sure the beakers are thoroughly cleaned after each test.
· Use same paper in each test.
· If the paper gets wet, change the paper, but same kind.
· Make sure the same person is recording the time, as reaction times
differ in people.
Method:
1.Take two 200ml beakers and fill one with hydrochloric acid and the
other with sodium thiosulphate, label each beaker.
2.Using a large measuring cylinder (100ml), pour 90ml of sodium
thiosulphate into it and fill the rest with water, so that it reaches
100ml.
3.Pour sodium thiosulphate and water into conical flask and place over
lined paper.
4.Measure 10ml of hydrochloric acid into small measuring cylinder.
5.Pour the hydrochloric acid into the conical flask containing sodium
thiosulphate and water, begin timing. Stop timing as soon as the lines
of paper are no longer visible through conical flask.
6.Record time into table.
7.Wash out conical flask and large measuring cylinder, otherwise it
Then titrate with the sodium thiosulfate solution as in the standardization procedure, adding 6 drops of starch indicator near the end of the titration. Record the volume of thiosulfate solution used in the titration. Make a duplicate
The rate law determines how the speed of a reaction occurs, thus allowing the study of the overall mechanism formation in reactions. In the general form of the rate law, it is A + B C or r=k[A]x[B]y. The rate of reaction can be affected by the concentrations such as A and B in the previous equation, order of reactions, and the rate constant with each species in an overall chemical reaction. As a result, the rate law must be determined experimentally. In general, in a multi-step reaction, there will be one reaction that is slower than the others.
reaction is the rate of loss of a reactant or the rate of formation of
Experiment is to investigate the rate of reaction between hydrochloric acid and calcium carbonate Hydrochloric acid + Calcium Carbonate Þ Calcium Chloride + Water + Carbon Dioxide 2HCl (aq) CaCo3 (s) CaCl2(s) H2O (aq) CO2 (g) There are a number of variables in this experiment and these are listed below as input variables and outcome variables.
Ø The length of the magnesium ribbon will have to be kept to 0.03g on
It is important however to note that the NH4 and K ions are still in
In a 250ml beaker place 100mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved. After 1 minute measure the temperature and record it, do this for a further 2 minutes (3 minutes in total). Repeat this process for a total of 10 teaspoons.
Investigating How Changing the Concentration of Hydrochloric Acid Affects the Rate of Reaction with Sodium Thiosulphate Solution
2. In the large beaker, put water and boil it completely. After that, remove the beaker from heat. 3. Sample tubes (A-D) should be labeled and capped tightly.
Chemical kinetics is the study and examination of chemical reactions regarding re-arrangement of atoms, reaction rates, effect of various variables, and more. Chemical reaction rates, are the rates of change in amounts or concentrations of either products or reactants. Concentration of solutions, surface area, catalysts, temperature and the nature of reactants are all factors that can influence a rate of reaction. Increasing the concentration of a solution allows the rate of reaction to increase because highly concentrated solutions have more molecules and as a result the molecules collide faster. Surface area also affects a
One vital process in the human body observed in chemistry is the idea of chemical kinetics. Chemical kinetics is the study of the rate of reactions, or how fast reactions occur.1 Three factors that affect chemical kinetics are concentration, temperature, and catalysis. As the concentration of a substance increases, the rate of the reaction also increases.1 This relationship is valid because when more of a substance is added in a reaction, it increases the likelihood that the
And the symbol equation for it is:. Na2S2O3 + 2HCl, S + SO2 + 2Na + H2O. Before conducting my experiment, I will research into, amongst other things, the factors that affect the rate of a reaction. This is so that I may have enough information to understand the effect of temperature on the rate of a reaction and also gain appropriate understanding to make a suitable prediction as to what the outcome of my experiment will be. Reactions occur when the particles of reactants collide together continuously.
We must also make sure that we add both the water and the sodium thiosulphate at exactly the same time (into the beaker with the hydrochloric acid in it), or it could affect the results of the experiment. We must start the stopwatch at the exact time as we put the water and the sodium thiosulphate into the beaker. To do this, it is a lot easier if there are two people doing the experiment, so one person can put the two substances in the HCL, and one person can start the stopwatch. Also, the person timing the experiment will look for the disappearance of the cross, otherwise there would be a time lapse between seeing the cross disappear and telling the other person to stop the clock and then eventually stopping the clock. It is also important to keep the temperature the same to obtain fair results, however we do not have to worry about this as the temperature will be kept at room temperature throughout the experiment.
The rate of reaction is how quickly or slowly reactants in chemical reactants turn into products. A low reaction rate is when the reaction takes a long time to take place; hence, a reaction that occurs quickly has a high reaction rate. A rate refers to how slow or quick the product is produced. It is possible to control the rate of chemical reactions and speed up or slow down the rate of chemical reactions by altering three main factors which are temperature, concentration and the surface area. When the temperature of the reactants increases, the molecules vibrate at a more intense speed therefore colliding with each other more frequently and with increased energy resulting in a greater rate of reaction. Accordingly, as the temperature decreases the molecules will move slower, colliding less frequently and with decreased energy resulting in the rate of reaction decreasing. Concentration is how much solute is dissolved into a solution and is also a factor that affects the rate of reaction. When the concentration is greater this means there is an increased amount of reactant atoms and molecules resulting in a higher chance that collisions between molecules will occur. A higher collision rate means a higher reaction rate. Consequently at lower concentrations there are reduced chances of the molecules colliding resulting in a lower reaction rate. The measurement of how much an area of a solid is exposed is called the surface area. The quicker a reaction will occur the more finely divided the solid is. For example, a powdered solid will usually have a greater rate of reaction in comparison to a solid lump that contains the same mass for it has a lower surface area than the powdered solid.
tube. Add 6 mL of 0.1M HCl to the first test tube, then 0.1M KMnO4 and