The increase in the temperature will affect the rate of dissolving by speeding up the process. The solvents are able to move faster in higher temperatures which results to a fast process of dissolving. How does stirring affect, how fast sugar dissolves in water? When a sugar cube is solid, all the particles are tightly packed together. As it begins to dissolve, the particles begin to move apart.
Both mole of HCL(the 2 moles of HCL and the 1 mole of HCL) have less energy , and thus when the 3 moles of HCL reacts with Mg, there is even more energy between the Mg and the HCL particles, so hence the rate of the reaction will be faster. Sources of Error: What could have been done is more trials to make sure
Reaction rate is affected by any catalysts present (which speed up the reaction usually with an intermediate step), temperature (increases the number of particles collisions), concentration (increases the number of collisions), and surface area (increases the space available for collisions). Reactions can only occur when collisions take place. The most generic form of the rate law is Rate = K * [A]m * [B]n where (k is a constant specific to an equation and temperature). Now, the compounds A and B might not have any effect on the rate, which would cause them to drop out of the equation completely, or they might have so much effect that they are raised an order (squaring the concentration). The rate law for this reaction is k [CV+]m[OH-]n. Since the hydroxide ion concentration at the beginning is about 1000 times larger than the concentration of crystal violet, [OH-] will not change that much during this
Neutralisation is an exothermic reaction, as a result of this the heat is given out because of the energy released from the forming bonds is greater than that taken in and used in the breaking of the bonds. The heat which gives off in the reaction can be measured by changing it into joules of energy. The heat produced during neutralisation is because of the reaction of acid and alkali to produce 1 mole of water. In an exothermic reaction the products have a lower energy than the reactants, because energy is lost during the reaction. * If there is a rise in the temperature, then the reaction is exothermic and involves a negative enthalpy change.
Whether the strength of Hydrochloric acid will affect the speed of the rate of reaction when reacting with Magnesium Ribbon. I want to find out whether the strength of Hydrochloric acid will affect the speed of the rate of reaction when reacting with Magnesium Ribbon. Variables There are two important independent variables in my investigation the first of which is the concentration of the Hydrochloric Acid used during the investigation. The concentration of the acid will partly determine how fast the reaction takes place, if we put some of the magnesium ribbon into the HCL at 2molar then it might have simply dissolved within a few seconds and then I would not have had time to record down any decent enough results to plot a graph with. The other important independent variable that will affect the speed of the rate of reaction is the length of magnesium ribbon.
This method is used because it has two certain advantages, according to Nerdz-Stormes. First, the percentage of quantity of the yield is much higher with this method than if it is just manually pressed. Second, it’s aimed to get a lower boiling point of the liquid by mixing the compound with water. The theory of this distillation process is mixing compounds that contain the aimed product with water to reduce the boiling point of it, so the organic compound does not decomposed by heat. The boiling point can be reduced because of the vapour pressure of it would be the sum of water’s vapour pressure and the compound’s vapour pressure.
The particles in the higher temperature move faster than when they are in a colder temperature. The pressure in the higher temperature is higher because this means that there are more pushes in an area. Yes there is a relationship between pressure and volume. The graph shows that for every -.300 KPa there is 1 mL. This means that in more space the same # of particles will push less.
3.2 Hypothesis – When the tablet is heated the particles move around faster dissolving the tablet. 3.3 Prediction – The hotter the tablet the faster the tablet will dissolve within the Hydrochloric Acid. 3.0 Experiment Design 4.4 Variables and Controls Type Of Variable | Independent | Dependant | Controls | Characteristics: | Temperature of Tablet | Time taken for acid to react with tablet | * Same size beaker * Same Stopwatch and timer * Same amount of hydrochloric acid * Same number of tablets | Reason | The difference in temperature has been changed deliberately with the Bunsen burner. | The time will vary due to how fast the hydrochloric acid breaks it down. | The variables must be controlled so the experiment is a fair test otherwise the experiment is not accurate.
The reason for this I concluded, was the collision theory. At the higher molarities of Potassium Iodide there were too many moles and therefore too many collisions were happening. Therefore the product was being made almost instantly. When I reduced the concentration of the reaction this meant there were less particles of iodide in the system so the reaction was happening slower. I also lowered the concentration of Hydrogen Peroxide 0.017M.