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the effect of the temperature on the reaction rate
rate of a reaction experiment
rate of a reaction experiment
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Rates of Reaction
Planning
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To measure the rates of reaction three variables were used. Firstly, a
basic experiment was set up this was a delivery tube connecting a test
tube filled with water in a bowl of water to a flask with calcium
carbonate with a solution of hydrochloric acid. Various sizes of
calcium carbonate was used (large, medium and powered particles) each
variable was tested 4 times. As the particles and acid were mixed
together the time was recorded to see how long the mass (test tube of
water) took to decrease. The time was recorded at every 2cm³ interval.
The results collected were the seconds the mass decreased to 2cm³,
4cm³, 6cm³ 8cm³ and 10cm³. The different particles are varied to show
if the surface area has an effect on the rate the reaction.
The second variable was the concentration of the acid. The same
experiment was carried out but this time the practical used different
molars of the acid (2molar, 1 molar and 0.5molar). As the same size
particles were added each time a different molars of acid was added
with the particles. The time was recorded at each 2cm³ interval.
Several experiments were carried out using different molars to compare
the results. Varying the concentrations helps to prove a higher molar
of acid reacts faster.
The third variable was temperature this was completed in the same way.
Before the acid was mixed with the calcium carbonate the acid was
heated up at different temperatures using a bunsen burner. The three
different temperatures the acid was heated at were 25ºc (room temp),
35ºc and 45ºc. The results collected were the times recorded each time
the mass decreased every 2cm³ intervals. The temperatures will change
because differences in temperatures will show if the rate of the
reactions increases or decrease.
Equation:
Calcium carbonate + Hydrochloric acid à Calcium chloride + Carbon
dioxide+ water
Equipment:
Calcium carbonate particles - (larger, medium and powder)
Hydrochloric Acid - (2m, 1m, 0.
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.
It is important however to note that the NH4 and K ions are still in
Investigating Rates of Reactions My aim is to investigate what factors affect the rate of reaction between magnesium and hydrochloric acid. The factor that I will be focusing on is the concentration of Hydrochloric acid. [IMAGE]Reaction Equation: Mg (s) +2HCl (aq) = MgCl2 (aq) +H2 (g)
Investigation to find out if changes in concentration of acid affect the rate of a chemical reaction
In this experiment there five different phases and in each a different factor of the Collision Theory was tested. The first phase was called, Nature of the Reactants and it had three parts to it. In the first part of it which was steps 1-4, 5 pieces of mossy zinc were put into 3ml of 2M H_2 〖SO〗_4 and during this time bubbles were produced. After a few minutes the zinc was removed from the acid and it was now clean zinc.
because I think it will give a wide set of results to put into a
The Effect of Concentration on Reaction Rate Introduction I will be carrying out an investigation into how concentration affects reaction rate. I will be looking at sodium thiosulphate and hydrochloric acid. The reaction is represented by the following equation: [IMAGE]Na2S2O3(aq) + 2HCl(aq) 2NaCl(aq) + H2O(l) + SO2 (g) + S (s) I will add the hydrochloric acid to the Sodium Thiosulphate and time how log it takes for the mixture to turn opaque. I will use a different concentration of Sodium Thiosulphate each time. Prediction
In order to find a good set of results for this experiment I need to
being used up, for that is a property of a catalyst is, it speeds up a
Investigation looking At the Speed of Reactions Introduction The aim of this experiment is to find out how a variable can affect the results from a scenario set up in scientific environment. The experiment is to see how a certain variable will affect the amount of Gas produced from a Calcium Carbonate and Hydrochloric Acid Reaction. The Science Calcium Carbonate is a generally white or colourless mineral that is translucent.
Investigating Factors that Affect the Rate of Reaction There are certain factors which affect the rates of reaction in an experiment. These factors are: · Pressure · Temperature · Concentration * Surface area / particle size and * The addition of a catalyst The factors that I will be concentrating on are temperature, concentration and surface area / particle size. Pressure Pressure influences the rate of reaction only when the reactants are in their gas phase. Pressure does not affect them much when they are either solids or liquids.
Some terms and ideas that will explored in this experiment are the rate of a chemical reaction and seeing how it is affected by the concentration of the reactant or reactants. Reactant concentration is the strength of the solution. The way reactants concentration affects the reaction rate is commonly known as the rate law. "The rate law can only be experimentally determined and can be used to predict the relationship between the rate of a reaction and the concentrations of reactants,"(Holt 2006). To understand or determine the rate of this chemical process one can make an educated guess about the reaction mechanism. "The reaction mechanism is the way in which a chemical reaction takes place, expressed in a series of chemical equations. A reaction that involves a single reactant, the rate is often proportional to the concentration of the reactant raised to some power” (Holt 2006). Rate= k [reactant]n is the formula used when determining rate law. The order of the reaction is represented by the exponent n. Based off the of the number of molecules that enter the...
Throughout the experiment the reaction time of the reactants will be recorded under different temperature environments. The hypothesis of this experiment is that the reaction rate of the reactants will increase as the temperature increases which means that the reaction time would be shorter (faster) as the temperature increases. To justify the accuracy of the hypothesis, the chemical equation of the experiment was examined and studied to predict the products after the chemical reaction; the chemical equation
The effect of concentration on the rate of reaction between sodium thiosulphate and dilute hydrochloric acid
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.