Wait a second!
More handpicked essays just for you.
More handpicked essays just for you.
Reaction Of Magnesium With Hydrochloric Acid
Rate of reaction investigation
Reaction rate experiment
Don’t take our word for it - see why 10 million students trust us with their essay needs.
Recommended: Reaction Of Magnesium With Hydrochloric Acid
Investigation of Rates of Reaction I am going to investigate the rate of reaction with magnesium and
different concentrations of hydrochloric acid. In order to carry out
the experiment, I will need the correct apparatus which are:
* Goggles
* Stop clock
* Beaker
· 30 cm3 measuring cylinder
· 5x70mm magnesium ribbons
· 1, 1.5, 2, 2.5, 3 mol./dm3 hydrochloric acid
· Gas syringe
Next, the apparatus has to be set out, which should look like this:
[IMAGE]
Key Factors:
The magnesium has to be sanded to remove any oxide on the ribbon.
This improves a fair test. The hydrochloric acid must be handled
safely as it is hazardous. The pipe connecting the gas syringe and
beaker together should not have any holes from previous use as the
Objective: The objective of the experiment is to determine what factors cause a change in speed of a reaction. It is also to decide if the change is correlated with the balanced equation of the reaction and, therefore, predictable. To obtain a reaction, permanganate, MnO_4^(1-), must be reduced by oxalic acid, C_2 O_4 H_2. The balanced equation for the reaction is:
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.
We began this investigation by suiting up in lab aprons and goggles, we then gathered our materials, found a lab station and got to work. We decided to start with the magnesium in hydrochloric acid first, we measured out 198.5 L of HCl and put it in the foam-cup calorimeter and took initial temperature reading. We then selected a piece of magnesium ribbon and found its mass: 0.01g. This piece was placed in the calorimeter and the lid was shut immediately to prevent heat from escaping. We “swirled” the liquid mixture in the calorimeter to ensure a reaction, and waited for a temperature change. After a few moments, the final temperature was recorded and DT determined.
It is important however to note that the NH4 and K ions are still in
9. When all magnesium has reacted, remove the lid and heat strongly for 5 minutes
The Effect of Temperature of Hydrochloric Acid on the Rate of Reaction Between Hydrochloric Acid and Magnesium
the acid was at 14 C the magnesium took 141 seconds to react and 27 C
Investigating the Rate of Reaction Between Marble Chips and Hydrochloric Acid I am investigating the rate of reaction between marble chips (calcium
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.
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.
Kinetics is the discovery and study of the reaction rates of chemical reactions. These reaction rates involve the pace or rate at which a reaction progresses. Many specific conditions can affect the reaction rate value; furthermore, the factors include the concentration of the reactants, the polarity of the solvent, and temperature1. The rate of reaction can be determined and studied using a rate law, an equation that correlates the rate with concentrations and a rate constant. This experiment’s reaction involving t-butyl chloride has a first order reaction rate, which means that the reaction’s rate law equation is the first order equation shown below.
The aim or purpose of this investigation is to explain how concentration affects the rate of reaction (the decomposition of sodium thiosulphate in reaction with hydrochloric).
On a two pieces of paper, we drew a cross and place a beaker on top of
Investigating the Effects of Temperature on the Rate of Reaction between Magnesium and Hydrochloric Acid Introduction Chemical kinetics is the study and examination of chemical reactions regarding re-arrangement of atoms, reaction rates, effect of various variables, and more. Chemical reaction rates, are the rates of change in amounts or concentrations of either products or reactants. Concentration of solutions, surface area, catalysts, temperature and the nature of reactants are all factors that can influence the rate of reaction. Increasing the concentration of a solution allows the rate of reaction to increase because highly concentrated solutions have more molecules and as a result the molecules collide faster. Surface area also affects reaction rate because when the surface area of a reactant is increased, more particles are exposed to the other reactant.
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.