Gcse Chemistry Coursework On Rates Of Reaction

Gcse Chemistry Coursework On Rates Of Reaction-79
The factors to discuss might be: amount of limestone? (1) its the hydrogen ion, H (aq), is the active ingredient that actually 'attacks' the metal or carbonate, and acids can ionise to different extents, (2) 1 molar or 1 mol dm-3 (1M) H2SO4 is twice as acid as 1M HCl because each H2SO4 provides 2 H 's whereas each HCl just 1.If you have decided, for example, to investigate the effect of acid concentration on the speed of a reaction, then everything else should be kept constant for a fair test, and this should be obvious in your plan for the reasons discussed above!

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Hence, these results show that an increase in concentration increases the rate of a reaction.

As you can see, the greater the concentration of the acid used in a reaction the steeper the curve and the shorter the reaction time.

Both the Sodium Thiosulphate and Hydrochloric acid are soluble in water; therefore the concentration of either can be changed.

However I have chosen to vary the concentration of the Sodium Thiosulphate as it is available to me in larger amounts and is more practical for my investigation.

* Put the test tube rack into the water bath at a temperature of 40o C so the temperature doesn't affect the results as it is also a variable.

* Wait ten minutes to insure that both of the substances are at 40o C.You can continue in a broader context by introducing some background theory and descriptions of the factors or VARIABLES which may have an effect on the rate of the reaction you are studying (include briefly factors which might not apply). Is there any other factor for the reaction you are studying?In your 'method' description use the correct units or descriptors. will any of the reactants or products be affected by change in temperature or pressure? there are several reasons why the same acid should be used if its a reactant in the investigation, e.g.The rate is measured by dividing one by the time the reaction took to take place.There are five factors that affect the rate of reaction: Temperature Concentration (of solution) Pressure (in gases) Surface area (of solid reactants) Catalysts I have decided to investigate the effect of concentration on the rate of reaction as I feel that it is manageable to measure, will show clear results and is much more practical than the other five variables. If we take the reaction between magnesium and hydrochloric acid, in order for them to react together: 1. In concentrated acid there are more acid particles, therefore there is a greater chance of an acid particle hitting a magnesium particle. Before, we discover the reasons for the above causing an increase in rate, we must first look at what is needed to cause a reaction to occur! The rate of a reaction depends on how many successful collisions there are in a given unit of time. This means there is less chance of an acid particle hitting a magnesium particle as compared with acid of a higher concentration.Diagram of experiment: My prediction If the concentration of a solution is increased there are more reactant particles per unit volume. Conclusion For this to fully make sense it is necessary to recap the collision theory briefly: For a reaction to occur particles have to collide with each other. If the frequency of collisions is increased the rate of reaction will increase.However the percentage of successful collisions remains the same.* Look straight down the top of the beaker and you should be able to see the cross, you should stop the stopwatch when the substance becomes so cloudy that you can no longer see the cross.You should repeat this experiment for each of the concentrations that are needed varying the water and sodium Thiosulphate as you go. Only particles with enough energy to overcome the barrier will react after colliding.

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