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The Effect of Concentration on Reaction Rates
Temperature effect on rate of reaction
Rate of reaction chemistry lab
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Recommended: The Effect of Concentration on Reaction Rates
Rate of Reaction Investigation
Aim:
To investigate the effect of concentration upon the rate of reaction
between Sodium thiosulphate (Na²S²O³) and dilute Hydrochloric acid
(HCl). This is:
Na²S²O³ + HCl 2NaCl + H²O + SO² + S
This experiment will be done in two parts. Firstly the experiment will
be done with the volume of HCl and total volume constant, and changing
the Thiosulphate and water volumes, thereby changing the concentration
of the thiosulphate. The second part of the experiment will be keeping
the thiosulphate and total volume constant and changing the HCl and
water volumes. The indicator for the rate of reaction is the sulphur
deposit left by the reaction, and when it covers a cross on a piece of
paper, the timing is stopped.
Theory:
I believe that the weaker the concentration of the thiosulphate, the
slower the rate of reaction. This is because of collision theory. In
collision theory there are three main things that affect the collision
of atoms in a reaction and thus the rate of reaction, temperature of
reagents, surface area of reagents and the concentration of the
reagents. For concentration (which is the part which is being
investigated) it says that the higher the concentration of the
reagents, the quicker the rate of reaction. I also believe that the
weaker the acid concentration, the slower the rate of reaction. This
is also because of collision theory. I also believe that changing the
concentration of the thiosulphate will have more of an effect on the
reaction time, as this is the reagent that reacts to give the sulphur
used for indicating the reaction time.
Method:
1) Set up apparatus as in diagram. (Note protective goggles must be
worn at all times)
2) Add 10cm³ of Na²S²O³ and 40cm³ of water. (Measured by measuring
cylinder)
3) Add 10cm³ of HCl and start timing the reaction. When the deposits
cover the cross, stop timing.
4) Repeat experiment with other values for Na²S²O³ and water, keeping
Experiment is to investigate the rate of reaction between hydrochloric acid and calcium carbonate Hydrochloric acid + Calcium Carbonate Þ Calcium Chloride + Water + Carbon Dioxide 2HCl (aq) CaCo3 (s) CaCl2(s) H2O (aq) CO2 (g) There are a number of variables in this experiment and these are listed below as input variables and outcome variables.
Ø The length of the magnesium ribbon will have to be kept to 0.03g on
It is important however to note that the NH4 and K ions are still in
Obtain a sample of metal that has been immersed in boiling water and place it in the cup of water.
Chemical kinetics is a branch of chemistry that involves reaction rates and the steps that follow in. It tells you how fast a reaction can happen and the steps it takes to make complete the reaction (2). An application of chemical kinetics in everyday life is the mechanics of popcorn. The rate it pops depends on how much water is in a kernel. The more water it has the quicker the steam heats up and causes a reaction- the popping of the kernel (3). Catalysts, temperature, and concentration can cause variations in kinetics (4).
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
Determine the reaction order for Na2S2O3 using calculations described in the Background. Show your work. Note that your answer will probably not be an even whole number as it is in the examples.
== == = The formula for the chemical reaction is: = ==
== Refer to, Chemistry Lab #1 – What’s the substance? I didn’t change most materials when I did this experiment, but I added 4 materials, which are: * 5 test tubes * 2 stoppers * 1 large piece of paper And I deleted 1 material, which is: * Spatula Methods = == ==
== In this experiment I shall be varying the volume of sodium thiosulphate, hydrochloric acid and water, and measuring the reaction rate. When I increase the amount of sodium thiosulphate with less water, I think the time for the cross to disappear would be faster than there would be with little sodium thiosulphate and more water – taking in account the amount of hydrochloric acid is the same. The reason why I think this is because the particles in the solution that will collide. There is a theory called the collision theory, and some of the factors from this, may affect the reaction rate in my experiment.
The initial hypothesis held true when compared to the results acquired within the experiment. By completing the experiment it was found that the concentration of sodium thiosulfate was inversely proportional to the time take for the cross to disappear.
has on the rate of reaction. I will do this by recording the time it
And the symbol equation for it is:. Na2S2O3 + 2HCl, S + SO2 + 2Na + H2O. Before conducting my experiment, I will research into, amongst other things, the factors that affect the rate of a reaction. This is so that I may have enough information to understand the effect of temperature on the rate of a reaction and also gain appropriate understanding to make a suitable prediction as to what the outcome of my experiment will be. Reactions occur when the particles of reactants collide together continuously.
We have no gases and solids involved, therefore it is easy to deal with solutions. Similarly, the use of a catalyst complicates things, and if used incorrectly could alter the outcome of the experiment. The theory behind this experiment is that increasing the concentration can increase the rate of the reaction by increasing the rate of molecular collisions. GRAPH I will place the reaction mixture on a paper with a black cross drawn on it. When the cross is completely obscured, the reaction will be finished.
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.