Investigating Reaction Rates of Sodium Thiosulphate and Hydrochloric Acid

What is the appearance of reactant, Evidence of chemical reaction, and properties of a product?

This website was used on October 3, 2014 to help develop a better understanding of collision theory in order to explain the various factors affecting the rate of reaction.

The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

How concentration affects the rate of reaction between Hydrochloric Acid and Sodium Thiosulphate Chemistry Coursework How Concentration Affects a Reaction Aim: The aim of this experiment is to find out how concentration affects the rate of reaction between Hydrochloric Acid and Sodium Thiosulphate. Introduction: This experiment will be carried out by drawing a cross on a piece of paper and mixing hydrochloric acid and sodium thiosulphate together to see if the cross disappears. The concentration of hydrochloric acid would change every reaction to show that concentration effects a reaction.

Which means that no starch-iodine colour will appear until all the thiosulphate has been used up. The amount of time taken for this occur (and the reaction to suddenly turn blue) is the same amount of time for the reaction to produce the equvilant amount of Iodine.

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,

This report discusses how varying the mole ratio of the reactants affects the amount of the product that is produced and the amount of the reactants that remain at the end of the chemical reaction. We know that you can’t simply add another atom of nitrogen and take an atom of hydrogen away from ammonia because it would change to another substance. We also know that in a chemical reaction atoms cannot be created or destroyed but can make a new substance. A guiding question was made so they can figure out how to solve/find out what is going on. The atomic theory is connected to this lab because that the atoms in the lab cannot be created of destroyed during a chemical reaction. Meaning that each side the of the equation must include the same number of each type of atom. The relationship between the amounts of any two compounds, in moles, that are involved in a chemical reaction. In this lab we are showing how different ratios of moles of sodium bicarbonate and acetic acid and how the different moles leave and percentage out of the product but still remains in the lab. How this lab works we will combine sodium bicarbonate and acetic acid and we are see the amount of CO2 leftover after the reaction happens. Knowing this.

The purpose of this experiment is to study the effect that inhibitors, light intensity, and wavelength have on the rate of the Hill Reaction. This was completed by the use of isolated chloroplasts retrieved from spinach leaves using a modification of a standard fractionation procedure, the substances were then then placed under a light source to be tested for the effects of different inhibitors, varying distance away from a light source, and different colored light filters. Overall, it was shown that no light source at all and the presence of inhibitors had a more negative effect on the reaction and that as distance from the light source increased, the rate decreased. In the wavelength reaction, the reaction reacted less in the presence of a green or yellow light than the red or blue filters. These findings seem to match what was expected based on the knowledge of how photosynthesis and the Light and Dark Reactions.

Throughout the experiment, countless calculations were made to calculate the enthalpy of formation for magnesium oxide. This was accomplished, first by finding the temperature change through use of a temperature probe within a chemical reaction with magnesium and hydrochloric acid, along with a chemical reaction containing magnesium oxide and hydrochloric acid. For the reaction that consisted of magnesium and hydrochloric acid, the temperature change was much more rapid compared to the reaction between magnesium oxide and hydrochloric acid. The reaction was gray in color, steamed, bubbled, and had a strange smell (likely consisting of the released hydrogen gas). In comparison, the reaction between magnesium oxide and hydrochloric acid was lackluster, producing no bubbles and staying relatively clear in color. Although most magnesium and magnesium oxide went from the weigh boat into the reaction, not all did, potentially affecting our final results.

Stoichiometry is the numerical relationship between products and reactants;from its calculations, one can predict the products when only the reactants are known or vice versa. Most calculations in chemistry use this in some way (Graves, 2013). Along with stoichiometry, dimensional analysis can also be used, and through the use of both one can calculate the moles of a substance, limiting reagents of a reaction- the substances that limit a reaction’s potential yield, substances that are in excess, number of atoms of a substance, analysis of a combustion reaction,and the molarity of a solution (Burdge and Overby, 2012).

If mass or gaseous volume of one of the reactants or products in a chemical reaction is known, mole(s) or mass or gaseous volume of a reactant or product can be calculated involving the mole ratio of a chemical equation.

In this section we had to show what the molecules look like before and after chemical reactions. I then had to write how I knew it was a chemical reaction or how I knew it was not a chemical reaction. Electrolysis is a chemical reaction. This is where the real growth happened for me. Not only did I know what happened to atoms and molecules in a chemical reaction, but I could also identify one and say why it was a chemical reaction. A chemical reaction is when one or more substances combine/decompose to create a new substance(s). I was also able to show I knew what reactants and products are. A reactant is a substance that is present before the chemical reaction. It is part of the “old” stuff that will have its atoms rearranged into a new substance. That brings me to product. A product is the new stuff that has formed as a result of the atoms rearranging. Knowledge of all of these terms and concepts helped me get the question

Rate of Reaction Using Enzymes In this bit of coursework I will be investigating the rate of reaction in which enzymes are the catalyst breaking down a substrate. The substrate I am going to use is Hydrogen Peroxide (H2O2, water with another Oxygen), this molecule usually breaks down on its own accord, but also the rate of decomposition can be increased with the use of a catalyst; in this case the catalyst is a biological one called an enzyme. Hydrogen Peroxide slowly breaks down on its own accord into water (H2O) and oxygen (O2): 2 H2O2 à 2H2O + O2 Hydrogen Peroxide à Water + Oxygen

By looking at the graph one can say that by looking at the shape of