RATES OF REACTION Formative.....
Click here for an examplar of a METHOD
NB You must write down the different temperatures in your trials in your method
Conclusion:
You MUST refer to your aim/purpose AND use the same language !!!
ie: you must use key terms - TEMPERATURE and RATE OF REACTION in this conclusion.
I can conclude that ............ ***** ALWAYS*** justify with using your results !!!!!!
For TEMPERATURE - as the temperature of the reactants increases the rate of the reaction increases.
The 20 degree Celsius acid solution took an average of 350 secs to react with and dissolve the metal, whereas at 100 degrees Celsius acid solution the average time taken for the reaction to dissolve the metal was only 34 secs.
For CONCENTRATION - as the concentration of the reactants increases the rate of the reaction will increase
For SURFACE AREA - as the surface area of the reactants increases - the rate of the reaction also increases
DISCUSSION:
This is when you use your collison of particle theory
This is when you use your collison of particle theory
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• Fully explains that a greater surface area of calcium carbonate means there is an increased surface area for HCl to collide with, leading to a higher frequency of successful collisions and therefore a faster rate of reaction, linked to an observation.
Explains that the concentration of reactants is highest at the start, so there are more particles present and therefore there are more collisions occurring per unit time / collisions are more frequent and decrease as reactants decrease as reaction proceeds.
The concentration of reactants is highest at the start of the reaction, i.e. greatest number of reactant particles per unit volume at the start. As a result, there is a higher frequency of successful / effective collisions at the start and therefore a faster rate of reaction than later as reactants run out.
Fully explains that the reaction is faster at the higher temperature, because the particles have more kinetic energy / move faster. Therefore, there will be more frequent collisions, and these collisions will be more effective, as the particles will collide with more energy and same end point as same reactant mas
Explains that the concentration of reactants is highest at the start, so there are more particles present and therefore there are more collisions occurring per unit time / collisions are more frequent and decrease as reactants decrease as reaction proceeds.
The concentration of reactants is highest at the start of the reaction, i.e. greatest number of reactant particles per unit volume at the start. As a result, there is a higher frequency of successful / effective collisions at the start and therefore a faster rate of reaction than later as reactants run out.
Fully explains that the reaction is faster at the higher temperature, because the particles have more kinetic energy / move faster. Therefore, there will be more frequent collisions, and these collisions will be more effective, as the particles will collide with more energy and same end point as same reactant mas
The factor being investigated is surface area of the calcium carbonate / marble chips. In section A of the graph the rate is fastest as there are more collisions between the HCl and CaCO3. This is because at the start of the reaction there are more particles available for collision. In section B the rate of reaction is slowing down as the number of particles available for collision is becoming fewer as some of the HCl and CaCO3 have already collided and have been used up, therefore fewer particles and therefore fewer collisions. In part C the reaction has stopped, as all of the reactants (or one of them) have reacted, and therefore there are no particles present that can collide and react. The rate of Experiment 1 is faster as the slope in section A of the graph is steeper than in Experiment 2. It is faster because when smaller chips are used, the surface area of the chips is greater. Because there is more surface area, there is more surface for the HCl particles to collide. Because there are more collisions occurring more frequently, the rate is faster.
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