Rates of Reaction
Aim
I will be investigating the rate of reaction (how quick a reaction
takes) of Sodium Thiosulphate (Na2S2O3) and Hydrochloric Acid (HCl
{aq}). There are different variables that can affect the rate of
reaction. The different variables include Temperature, catalysts and
concentration. In this piece of coursework, I'll be analysing the
concentration.
The products we get are
Sodium Thiosulphate + Hydrochloric Acid --> Sodium Chloride + Water + Sulphur dioxide
Na2S2O3 (aq) + 2HCl (aq)--> 2NaCl (aq) + H2O (l) + SO2 (g) + S (s)
Apparatus
=========
1 Eye protection
2 measuring cylinders
1 White paper with bold black cross
1 Stopwatch
1 beaker (50ml)
Sodium Thiosulphate (0.2m)
Hydrochloric Acid (0.2m, 0.4m, 0.6m, 0.8m, 1m)
Prediction
==========
In my prediction I presume that if the concentration of Hydrochloric
Acid is increased, the faster the rate of reaction. The reason is
because of the collision theory. The collision theory is linked to all
the different variables that affect the rate of reaction. For a
reaction to occur particles need to collide with each other.
Unfortunately, only a small percent of particles collide to result in
a reaction. This is due to the particles overcoming the energy
barrier. The barrier is the activation energy or Ea. Particles need a
certain amount of energy to pass this barrier to successfully create a
reaction. For particles to get energy you can increase the temperature
to allow the particles to overcome this barrier. The activation energy
size depends on each sort of reaction.
Now the activation energy barrier has been passed, the percent of
successful collisions does not change. For this to change it now
depends on the different variables that affect the rate of reaction.
Concentration
-------------
When you increase the concentration this increases the amount of the
reactant particles per unit volume. Therefore there will be a higher
chance of the particles colliding with the opposing particles to
Cu (aq) + 2NO3 (aq) + 2Na+ (aq) + 2OH- (aq) → Cu(OH)2 (s) + 2Na+ (aq) + 2NO3(aq)
The equation shows how 1 mol of Na2CO3 reacts with 1 mol of H2SO4, so
Text Box: CaCO3 + HCl = CaCl2 + CO2 + H2O calcium carbonate + hydrochloric acid = calcium chloride + carbon dioxide + water
CaCl2 + H2O + CO2
It is important however to note that the NH4 and K ions are still in
Na2S203 (aq) + 2HCl (aq) -> 2NaCl (aq) + H20 (l) + SO2 (g) + S (s)
Abstract: This week we experimentally determined the rate constant k for the reaction 2HCl (aq) +Na2S2O3 (aq) → S (s) + SO2 (aq) + H2O (l) + 2NaCl (aq). In order to do this the average reaction time was recorded in seconds during two trials. The data from the experiment shows this reaction is in the first order overall: rate=.47s-1 [HCl]0 [Na2S2O3]1. These findings seem to be consistent with the expected results
== CaCO3(s) + 2HCC(l) CaCl2 (aq) + H2O(l) + CO2. = =
Total ionic- H+(aq) + Cl-(aq) + Na+(aq) + HCO3-(aq) → Na+(aq) + Cl-(aq) + CO2(g) + H2O(l) (Eq. 13)
Cl- (aq) + Na+ (aq) + OH- (aq) Na+ (aq) + Cl- (aq) +H+ + OH- [IMAGE]The above is an example of a neutralization reaction, involving an acid and an alkali. The result is a salt and water. In every neutralization reaction, the metal in the alkali (Na+ here) takes the place oh the hydrogen in the acid, forming a metal compound called a salt.
== == I completed a table to show my results, here is the table: Table 1. Results of different changes of substances Part A Copper (II) Sulfate and Water Reactant description Water (reactant): Color: Colorless Transparency:
If I were to roughly plot a graph for the reaction, it would look like
Hydrochloric acid + calcium carbonate arrow calcium chloride + carbon dioxide + water. HCl(aq) + CaCO3(s) arrow CaCl2(aq) + CO2(g) + H2O(l) Things that affect the reaction rate of this experiment are: 1. The temperature of the hydrochloric acid. 2.
Na2S2O3 (aq) + 2HCl (aq) → 2NaCl (aq) + S (s) + SO2 (g) + H2O (l)