Method:.
The first thing I have to is to check that all my pieces of magnesium are 2cm long or it will not be a fair test. The second thing I have to do is to measure 20cm2 of hydrochloric acid in to a beaker, and then I need to add the magnesium to the beaker, and then start the stop clock and then stop the stop clock when all the magnesium has disappeared. Then I will repeat the above steps for each of the different concentrations.
Explaining My Prediction:.
The collision theory is when particles must collide, and must collide with enough force to make a chemical reaction. To change the rate of reaction there needs to be more frequent collisions between particles, and also they need to collide with more energy. That is why this is my prediction is that the higher concentration on the acid, the faster the rate, because the higher the concentration means the more collisions, more collisions means faster reactions.
Safety:.
What to do to ensure safety from hydrochloric acid?.
Well as you hydrochloric acid eats away at substances, so to ensure safety I will wear goggles to protect my eyes, I will always be standing while I am doing my experiment in case there is a spillage, I will only use 2 molar acid.
What to do to ensure safety from hydrogen gas?.
Hydrogen gas is flammable so I will not let it be near a naked flame, where I am going to be using glass, there is a chance of it breaking, so I will take as much care as I can.
Results Table:.
Concentration of acid Time for Mg to stop reacting1 2 3 Extra readings if necessary Average time in seconds.
5m 849* 589 637 539 588.
75m 257 213 239 236.
1.0m 58 57 68* 58 58.
1.5m 32* 26 24 27 26.
2.0m 13 15 12 13.
* This sign means an anomalous result.
Simple Explanation:.
The simple explanation of this experiment is that the higher the concentration the faster the rate of reaction.
Trends and Patterns:.
The higher the concentration, the quicker the reaction.
For example:.
Chemical reactions are the heart of chemistry. ... Even the position of the reactants will affect the reaction rate. ... They cannot make impossible reactions occur, they only contribute to the reaction to increase the reaction rate. ... Inhibitors retard the reaction rate. ... The reaction rate can be controlled for observation by varying the intensity of the radiation. ...
Chemical reactions are the heart of chemistry. ... Even the position of the reactants will affect the reaction rate. ... They cannot make impossible reactions occur, they only contribute to the reaction to increase the reaction rate. ... Inhibitors retard the reaction rate. ... The reaction rate can be controlled for observation by varying the intensity of the radiation. ...
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At the end of a reaction the reaction rate slows down significantly as the reactants get used up throughout the reaction. Therefore the rate of reaction is greatest at the beginning of the reaction as there are more free reactant particles to collide with each other. ... The reaction rate will be quickest at the beginning because there are a lot of free reactants. As the reaction progresses the reactants will have been used up and fewer collisions will occur and hence the reaction rate will slow down dramatically. ... As the number of reactants doubles, the chance of a collision occurring betw...
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The rate of this reaction can be examined using a method called flash photolysis. ... An expression is then used to find the rate of reaction: Rate of reaction=k(O2)(O) K=rate constant (O2)(O)=concentrations of oxygen atoms and molecules. The rate constant depends on the temperature and pressure of which the reaction is happening and determine how fast it is going. ... This helps us understand the chemistry in the stratosphere as it tells us what is likely to be found there and what height the ozone is found at. ... A steady state is established between the rate of which Ozone is ...
