At the start, there are plenty of magnesium atoms and acid particles. I predicted that the more concentrated the acid solution the faster the magnesium and hydrochloric acid will react. The rate of reaction will depend on the rate of collisions between particles, we expect the rate of collisions Surface area of Magnesium ribbon: Then make up the different concentrations of acid.
Variables Operationalization of variables The dependent variables The duration of reaction, time taken for Magnesium to dissolve in hydrochloric acid completely measured using a stopwatch in seconds. I conclude that changing one factor does have a significant effect on the rate of reaction as we have seen.
I decided that it would be impractical to spend time on the following strengths of hydrochloric acid: The variables that could be used are: Therefore, this study intends to investigate the effect of concentration and surface area of reactants on the rate of chemical reactions.
It becomes MgCl which is soluble in solution so effervescence is seen as it dissolves and hydrogen is released.
Because The reaction was finished when the black cross on the pad dissapeared and this is only seen by the naked eye. I decided therefore that I would carry out each of the experiments.
I was right in my prediction but I did not predict that the rate of reaction slows down as time goes on which did happen in my experiment. I used the same size of magnesium, I also started the stop clock when the magnesium touched the acid and stopped it when the magnesium stopped fizzing for each experiment.
Background knowledge you should just write about different factors affecting rate like surface area, concentration or temperature depending on which one you are looking at and explain why, for example with temperature talk about the kinetic energy and collision theory.
Another factor that I learned is that the rate is constantly changing during the reaction because as time goes on there are fewer acid molecules. In this investigation I will test different concentrations of acid reacting with magnesium. This is pattern suggests that the reaction rate increase when the concentration of the acid increases because if you increase the concentration of the acid you are introducing more particles into the reaction which will in turn produce a faster reaction because there will be more collisions between the particles which is what increases the reaction rate.
We can work out the name of this gas by solving a simple equation: Rate of Reaction of Magnesium and Hydrochloric Acid Introduction In acid-base chemical reactions, there are four main variables, which influence the rate of reaction.
With the whole class doing this with different eye types, there is no exact fairness in the experiment. Therefore, we sought to test the duration of reaction of equal lengths Magnesium ribbons with reducing concentrations of hydrochloric acid. When the reaction takes place bubbles of H are given off, which might stay around the magnesium, which therefore reduces the surface area of the magnesium and so the acid cannot react properly so this affects the results.
Magnesium metal in form of a ribbon or powder reacts with acids rapidly than water liberating hydrogen gas. There are fewer acid molecules because when the acid reacts the same particle cannot react again, so there are less to end with than there are to start with. Reactants with high surface area provide a greater binding surface for other reacting molecules, and therefore increase the number of successful collisions at any moment.
The reaction is speeded up if the number of collisions is increased. The fastest reaction made was with no water, 60 cm of sodium this sulphate and 10 cm acid.
This will bring fairness to experiments to test all similar to rate of reaction. This reaction was very slow with a time of 4,4.Chemical reactions between substances are caused by the collision of particles.
More collisions mean a quicker rate of reaction. In the reaction between hydrochloric acid and magnesium ribbon, the chemical reaction takes place when the magnesium ribbon is dropped into the hydrochloric acid. [tags: GCSE Chemistry Coursework Investigation]. Aim The aim of this investigation is to find out how concentration of acid affects the rate of reaction between hydrochloric acid and magnesium ribbon.
EduCheer! Free Samples and Examples of Essays, Homeworks and any Papers Hydrochloric acid is a common laboratory acid.
Extracts from: a chemistry coursework from an Internet source and The. In the reaction between hydrochloric acid and magnesium, the hydrochloric acid will dissolve the magnesium and produce hydrogen gas.
All chemical reactions involve reactants which when mixed may cause a chemical reaction which will make products. In my case the reactants are hydrochloric acid and magnesium ribbon. Jun 05, · Rates of reactions between HCL and magnesium ribbon Aim I plan to investigate the effect of concentration of acid, in the reaction between dilute hydrochloric acid and magnesium ribbon.
The rate of a chemical reaction is a measure of how fast the reaction takes place. Apparatus To Investigate Magnesium Ribbon. Aim It is to tell how the reaction between magnesium and hydrochloric acid will be effected if we change the concentration of hydrochloric acid.
Introduction In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The balanced formula for this /5(2). Aim I plan to investigate the effect of concentration of acid, in the reaction between dilute hydrochloric acid and magnesium ribbon.
The rate of a chemical reaction is .Download