The Effect Of Sodium Thiosulphate On Reaction Rate

In reference to the collision theory, molecules act as small spheres that collide and bounce off each other, transferring energy among themselves when the collide. In order for a reaction to occur, there must be collisions between molecules. Through experimentation, factors are discovered that influence the reaction rates of chemical reactions include the concentration of reactants, temperature, surface area, the physical state of reactants, and a catalyst. This experiment regarding the factors that affect reaction rate tests the effects of increased concentration and

If the concentration of the solution is increased the particles have less room to move around which creates a greater chance of collisions. The surface area of the reactant greatly affects the speed of which it reacts because if the reactant is grinded up or cut up the solution has more room to get to it. The reaction rate can be calculated by the formulae; rate of reaction = total amount of reactant used or product made ÷ time taken. (Collision theory and rates of reaction, 2013)

As the concentration was increased, from 0.5 M, to 1.0 M, to 1.25 M hydrochloric acid, the time taken for 50mL of carbon dioxide to be produced significantly decreased, and from 0.5 M to 1.25 M it decreased by around 12 seconds.

Aim: The aim of this experiment is to observe how by increasing the temperature of sodium thiosulfate in a solution with 2.0 molar Hydrochloric acid can affect the rate of reaction and the rate in which a precipitate is formed.

Introduction: The rate of a reaction is the speed at which a chemical reaction happens. If a reaction has a low rate, that means the molecules combine at a slower speed than a reaction with a high rate. Some reactions take hundreds, maybe even thousands, of years while others can happen in less than one second. (Chem for Kids, 2016). Reactions require collisions between reactant molecules or atoms. The formation of bonds requires atoms to come close to one another. New bonds can form only if the atoms are close enough together to share electron. Higher temperatures make the collisions between molecules more violent. The higher temperatures mean higher velocities. This means there will be less time between collisions. The frequency of collisions will increase. (Chem, 1999) H2O2 is the chemical formula for hydrogen peroxide. The decomposition of hydrogen peroxide will break down into oxygen and water.

When the concentrations were changed so did the rate of reaction. When the concentration was changed to 0.265M the rate of reaction dropped by a factor of 0.5 (50%) below the control value. Furthermore when 60mL of water was added to the bleach dropping the concentration too 0.132M the rate dropped by a factor of 0.7 (70%).

There are many factors that can increase the reactivity of an element when mixed with hydrochloric acid. These include pressure, temperature, surface area and concentration.

8. The Hydrochloric Acid was carefully poured into the beaker with the Sodium Thiosulfate. Once the liquids had made contact, three seconds were waited until the stop watch was started.

Introduction: The rate expression for this reaction is of the form: rate = K(CV+)M(OH-)N Where k = re constant, m is the order of the reaction with respect to the concentration of CV+, and n is the order of the reaction with respect of OH-. In the experiment the concentration of OH- is purposely made 1000 times larger then Concentration of CV+. Thus, the concentration of OH- changes so little during the

To start off the experiment 25mL of water was placed into a labeled beaker and tested for the pH using pH test strips. Next the antacid tablet was placed in the solution and timed for how long it took to dissolve the tablet. Finally the temperature was measured. This same process was repeated for the acidic solution, and finally for the basic solution. After each experiment the pH, the reaction time, and the temperature of the beaker were recorded into a table. For this experiment the independent variable was the substance used (acid, neutral or base), and the dependent variable was the reaction time of each substance. The constant conditions of this experiment included the amount of substance being used, and the placing of one antacid tablet into each beaker. The experimental group was the acidic and basic solution, and the control group was the neutral

In this experiment we tested the effects that enzymes and substrate have on chemical reaction rates, which is the rate at which chemical reactions occur.. This experiment tested how different concentrations of enzyme and substrate affected the light absorption measurements on a spectrophotometer. The experiment also tested how temperature affected the light absorption, and in a separate test, the effect of the enzyme inhibitor hydroxylamine was also tested. In the first test conducted, 3 different concentrations of enzyme, and three different concentrations of substrate were measured in a spectrophotometer. For the enzyme and the substrate, the measurements got higher as the concentrations were higher, but the over measurements of the substrate were smaller than those of the enzyme. In the second test conducted, the medium concentration enzyme was tested under the temperatures; 4°C, 23°C, 37°C, and 60°C. The measurements in this test got higher as the temperature got higher, but did the measurements under 4°C were overall significantly higher than the other temperature measurements. Lastly, the last test conducted showed that the measurements of the substance with 0 and 1 drop of hydroxylamine inhibitor went up, but the measurements of the enzyme with 5 drops of hydroxylamine inhibitor stayed rather low and did not change much. In conclusion, these experiments showed that chemical reaction rates are sped up with higher concentrations of enzyme, substrate,

1. Describe what the results were. According to the results, the higher the concentration of sodium thiosulphate the higher the reaction rate. The graph above shows the reaction rate compared to the sodium thiosulphate solution is almost a straight line showing the relationship of the sodium thiosulphate and the rate of reaction.

A rate law is a mathematical equation that describe the rate of a reaction. A reaction rate is the change in concentration of reactants or products over time (3). A Vernier colorimeter was used to measure the absorbance (or concentration) of CV+ when mixed with OH. The concentration of CV+ generally decreased over time at a similar rate when mixed with 0.1M and 0.2M hydroxide. The data was copied into Excel then made into

The rate of a chemical reaction often depends on reactant concentrations, temperature, and the presence of a catalyst. Additionally, the rate law is determined mathematically only from experimental data. The reaction investigated in this experiment is:

This transformation relies on the amount of activation energy for the particle to form a new product, and the orientation at which the particles collide. There are several factors that can affect reaction rates within aqueous solutions including temperature, concentration, particle size and catalysts. Temperature affects the rate of reaction of a solution by adding heat which speeds up the particles within the solution or by slowing the particles down through the cooling of the reaction. Concentration also has a large impact on the rate at which a reaction occurs because of the change in the number of particles in the solution. By increasing the concentration of the reactants the collision frequency also increases which escalates the rate at which products are being formed. Decreasing the number of particles in the solution also will decrease the speed with which products are created. Once a reaction between substances has fully occurred, a dynamic equilibrium is established. Although in a dynamic equilibrium the concentration of the reactants appears to be unchanged, a reaction still occurs with the forward reaction rate being equal to that