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effects of concentration on reaction rate
the effect of temperature on the rate of a reaction
the effect of temperature on the rate of a reaction
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Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid
Rates of Reaction: Investigation
Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid.
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. The products are hydrogen gas and magnesium chloride.
The equation for this reaction is as follows:-
Magnesium + Hydrochloric acid Magnesium chloride + Hydrogen
Mg (s) + 2HCL (aq) MgCl2 (aq) + H2 (g)
Factors that affect the rate of reaction:-
* Temperature
* Mass of magnesium ribbon
* Concentration of hydrochloric acid
* Surface area of magnesium ribbon
I have chosen to use the concentration of hydrochloric acid as my independent variable. These different concentrations can be varied easily and made up accurately for the experiment.
Each experiment will be done four times so that an average reading can be calculated - ensuring an accurate and reliable conclusion. The measured variable will be the time taken for the same quantity of magnesium ribbon in each experiment to be used up in reaction. The constant variable will be the length of the magnesium ribbon used in each experiment.
Rate of reaction = Gradient of the line of a graph plotted with time taken to cease reacting against
concentration.
Concentration of a solution describes the number of active particles in a particular volume.
The unit of concentration is: mol.dm-3
Prediction
I predict that the higher the concentra...
... middle of paper ...
...ing around faster. This would mean HCL and magnesium particles would collide more frequently, thereby increasing rate of reaction.
I think that my results on graph 1 were suitable to draw an accurate best-fit line. The points are all joined by the line.
I used 5 different concentrations which were in a suitably wide range.
If I were to repeat the experiment I would use a slightly wider range of concentrations to expand my conclusion, such as 1.25M, 0.75M and
0.25M. If the resources were available, I would also extend the range to higher concentrations than the 2M I was restricted to in this investigation. Further investigation could also include using another factor as my independent variable.
I could differ the surface area of magnesium in my experiments, and see how this affects rate of reaction; in what way and if there is a definite proportional relationship.
This process is then repeated. In the second trial, the Mg ribbon did not completely dissolve and the results were thrown out. The third trial (referred to as the second in the following analysis due to the exclusion of the previous one) was successful, and measurements can be seen below. We then moved onto the second reaction using magnesium oxide and hydrochloric acid in the fume hood. We measured 200.1 mL of HCl and placed it in the calorimeter, and an initial temperature reading was taken.
The purpose of the experiment is to study the rate of reaction through varying of concentrations of a catalyst or temperatures with a constant pH, and through the data obtained the rate law, constants, and activation energies can be experimentally determined. The rate law determines how the speed of a reaction occurs thus allowing the study of the overall mechanism formation in reactions. In the general form of the rate law it is A + B C or r=k[A]x[B]y. The rate of reaction can be affected by the concentration such as A and B in the previous equation, order of reactions, and the rate constant with each species in an overall chemical reaction. As a result, the rate law must be determined experimentally. In general, in a multi-step reac...
Investigation of How Temperature Affects the Rate of Reaction of Sodium Thiosulphate and Hydrochloric Acid
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.
Input variables In this experiment there are two main factors that can affect the rate of the reaction. These key factors can change the rate of the reaction by either increasing it or decreasing it. These were considered and controlled so that they did not disrupt the success of the experiment. Temperature-
Rate of Reaction Between Marble Chips and Hydrochloric Acid. The aim of this experiment is to find out how different variables affect the rate at which the reaction between Marble chips (CaCO ) and Hydrochloric acid (HCl) is used. There are many variables that affect the rate of this reaction such as the following. 1.
the reaction; if it speeds it up, slows it down or changes it in any
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
The aim of my investigation is to find out whether the increase of temperature increases the rate of reaction between the two reactants of Sodium Thiosulphate and Hydrochloric acid. I will then find out and evaluate on how temperature affects this particular reaction. Factors There are four main factors, which affect the rate of reaction that are considered as variables for the experiment I will be doing, they are the following: Molecules can only collide when two of them meet together.
Hydrochloric acid + calcium carbonate arrow calcium chloride + carbon dioxide + water. HCl(aq) + CaCO3(s) arrow CaCl2(aq) + CO2(g) + H2O(l) Things that affect the reaction rate of this experiment are: 1. The temperature of the hydrochloric acid. 2.
The Effect of Concentration of Hydrochloric Acid on the Rate of Reaction with Magnesium Aim: To investigate the effect of concentration of hydrochloric acid on the rate of reaction with magnesium Prediction: As the concentration of the hydrochloric acid increases, so will the rate of reaction Hypothesis: In a reaction, particles of two different reactants react together to form a product. The reaction only takes place on account of two things, if the particles collide, and if the collision has enough 'activation energy'. The two reactant particles, in this case magnesium particles and hydrochloric acid particles, must collide with each other on the correct 'collision course'. If this does not occur then no chemical reaction will take place. The reaction must also have enough energy, this can be affected by temperature, the more heat the particles have the faster they move and so the more energy therefore more chance of successful collisions.
Dependent variables: The extent of the reaction (the time taken for magnesium to completely dissolve in HCL). The volume of hydrogen gas produced.
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
An investigation into how changing one variable influences the rate of reaction between marble chips and dilute Hydrochloric acid
My aim in this piece of work is to see the effect of temperature on the rate of reaction in a solution of hydrochloric acid containing sodium thiosulphate. The word equation for the reaction that will occur in the experiment is: Sodium thiosulphate + hydrochloric acid →, sulphur + sulphur dioxide +. sodium chloride + water ? where the sulphur is an insoluble precipitate.