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Concentration effect on rate of reaction results
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Recommended: Concentration effect on rate of reaction results
Reaction Rates
The 4 factors that control the rate of a reaction are:
* Concentration
* Temperature
* Surface area (substances size)
* Catalyst
CONCENTRATION.
In this experiment I am going to find out how the rate of reaction
between sodium thiosulphate and hydrochloric acid is affected by
changing the concentration.
REACTION: Sodium Thiosulphate + Hydrochloric acid
[IMAGE]Equation: Sodium Thiosulphate + Hydrochloric acid Sodium
Sulphate + Sodium Chloride + water + Sulphur + PPT
This reaction usually produces a yellow precipitate.
EXPERIMENT:
Dose changing the concentration of a liquid affect the reaction rate.
I will test this by putting Sodium Thiosulphate + Hydrochloric acid in
a conical flask which has a piece of paper under it with a black cross
on. As soon as I mix the Sodium Thiosulphate with the Hydrochloric
acid I will time how long it takes for the cross to disappear, the
faster the reaction the quicker the solution will cloud up so the
quicker the cross will disappear. I will then do the same experiment
but add water to the Sodium Thiosulphate to dilute it and time the
experiment again to see if there is any difference.
APPARATUS:
* Piece of paper with cross on it
* Measuring cylinder
* Conical flask
* Stop watch
* Thermometer
* Stirrer
METHOD:
1) Measure out 10cm3 hydrochloric acid in a measuring cylinder
2) Pour measured out hydrochloric acid in conical flask
3) Measure out sodium thiosulphate in a measuring cylinder from 30cm3
and no water to 5 cm3 of sodium thiosulphate and 25cm3 of water)
4) Pour in to conical flask so mixing with the Hydrochloric acid and
start top watch
5) Time how long it takes for the cross to disappear.
CONSTANTS: apparatus amount of hydrochloric acid
VARIABLES: amount of Sodium Thiosulphate and water
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The Effect of Concentration on Reaction Rate Introduction I will be carrying out an investigation into how concentration affects reaction rate. I will be looking at sodium thiosulphate and hydrochloric acid. The reaction is represented by the following equation: [IMAGE]Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + H2O(l) + SO2 (g) + S (s) I will add the hydrochloric acid to the Sodium Thiosulphate and time how log it takes for the mixture to turn opaque. I will use a different concentration of Sodium Thiosulphate each time. Prediction
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.