Rate of Reaction Investigation
Plan
In this experiment I will be investigating the rate of reaction and
the time taken for a 1cm strip of magnesium to entirely disappear in a
container of hydrochloric acid. The equation for this reaction is
magnesium + hydrochloric acid or
Mg(s) + 2HCL = MgCl2 (aq) + H2 (g)
For experiment my input variable will be the concentration of
Hydrochloric acid, so I will be using a concentration scale of 1-2 mol
dm-3.
My prediction is that the higher the concentration of hydrochloric
acid the faster the rate of reaction will be.
Below is a graph showing my predicted results:
I am basing my prediction on the premises that when the solution of
water and hydrochloric acid is dilute there are less hydrochloric acid
molecules in the solution. Making it is less likely that they collide
with the magnesium particles decreasing the speed of the reaction;
therefore the more concentrated the solution is the more hydrochloric
acid molecules there are and therefore there will be more reactions as
these molecules or particles collide with the magnesium. Collision
states that for a chemical reaction to occur particles must collide
with sufficient energy. The minimum energy required by particles is
known as the activation energy.
For this experiment I will require the following equipment:
Stop clock, measuring cylinder, syringe, beaker, hydrochloric acid,
sand paper, magnesium, diluted water and goggles.
The experiment will be set up as shown below:
· I will make the solution required using diluted water and
hydrochloric acid
· The concentration of this solution will vary as it is my input
variable
· The solution will be prepared in a beaker.
· I shall then sand down the 1cm magnesium strip so as to remove the
coating as it will affect the experiment and make it unfair.
· When the coating is completely removed I can drop the magnesium into
the solution at the same time as I start the stop clock.
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.
In a substance the rate of reaction will be quicker if it has a large
It is important however to note that the NH4 and K ions are still in
2. Clean the surface of a 20 cm strip of magnesium ribbon using steel wool
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)
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.
reaction is the rate of loss of a reactant or the rate of formation of
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.
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.
cloudy, to test this; I will place a piece of paper with a cross on
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.
Chemical kinetics is a branch of chemistry that involves reaction rates and the steps that follow in. It tells you how fast a reaction can happen and the steps it takes to make complete the reaction (2). An application of chemical kinetics in everyday life is the mechanics of popcorn. The rate it pops depends on how much water is in a kernel. The more water it has the quicker the steam heats up and causes a reaction- the popping of the kernel (3). Catalysts, temperature, and concentration can cause variations in kinetics (4).
with that is I would have to dilute the acid again as the times were
Rate of Reaction Experiment - Sodium Thiosulphate and Hydrochloric Acid To investigate the effect, of changing the concentration of a reactant, in a chemical reaction on it rate. The equation used for the experiment was: Sodium + Hydrochloric Sulphur + Sulphur + Sodium + water Thiosulphate acid dioxide chloride Na2S2O3 + 2HCl(aq) S(s) + SO(g) + NaCL(aq) + H2O The Collision Theory can explain reaction rates perfectly.
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.