Investigating The Rate Law And Activation Energy For 2hcl

Abstract: An ice calorimeter was used to study the reaction of magnesium metal and 1.00M

During the immersion of the magnesium metal in the hydrochloric acid solution, white bubbles could be seen escaping the surface of the metal as gas was produced during the reaction. Depending on the temperature of the hydrochloric acid and the overall molar concentration, the rate of reaction differed but the same signs were shown. During the reaction between the magnesium metal and higher concentrations of hydrochloric acid, it was observed that the test tube grew quite warm to the touch. As the immersed magnesium strip sank down, it appeared coated in a layer of white bubbles that fizzed like a carbonated drink. In the lower concentrations of hydrochloric acid, the strip spent some time floating at the surface of the solution in the test tube, later sinking down to the bottom as the

The purpose of this lab was to test the law of definite proportions for the synthesis reaction of combusting magnesium. In this lab, the polished magnesium ribbon was placed in covered crucible and was heated in order for it to react with Oxygen presented in air and in water provided. The result showed that Magnesium oxide formed through chemical reaction was made up of 60.19% magnesium and 39.81% oxygen, which is approximate proportion of both particles in every Magnesium oxide compound. From this lab it can be concluded that the law of definite proportion stating that the elements in a pure compound combine in definite proportion to each other is factual.

    In this lab, a calorimeter was used to find the enthalpy of reaction for two reactions, the first was between magnesium and 1 molar hydrochloric acid, and the second was between magnesium oxide and 1 molar hydrochloric acid. After the enthalpy for both of these were found, Hess’ law was used to find the molar enthalpy of combustion of magnesium, using the enthalpies for the two previous reactions and the enthalpy of formation for water. The enthalpy of reaction for the magnesium + hydrochloric acid reaction was found to be -812.76 kJ. The enthalpy of reaction for the magnesium oxide + hydrochloric acid reaction was found to be -111.06 kJ. These two enthalpies and the enthalpy of formation for water were manipulated and added together using Hess’s law to get the molar enthalpy of combustion of magnesium. It was found that the molar enthalpy of combustion of magnesium was -987.5 kJ/mol. The accepted enthalpy was -601.6 kJ/mol, which means that there is a percent difference of 64%. This percent difference is very high which indicates that this type of experiment is very inefficient for finding the molar enthalpy of combustion of magnesium. Most likely, a there are many errors in this simple calorimeter experiment that make it inefficient for finding the molar enthalpy of combustion of magnesium.

I could use a gas syringe to collect the gas that will evolve from my

About 80 mL of HCl was obtained and mixed with phenolphthalein. Using a LabQuest unit and Gas Pressure Sensor kit, the HCl mixture was added to the flask with the magnesium ribbon and allowed to react. When reaction was complete, the change of temperature and gas was recorded. This procedure was repeated for different masses of magnesium ribbon (masses found on page 89 of the lab manual). After the completed procedure, moles of H₂ produced in each trial were calculated. (The actual procedure can be found on pages 87-89 of the lab manual)

Because it is dangerous to burn magnesium, it is not possible to directly record heat change. Our lab team suggests an indirect way of determining the heat of combustion for magnesium. To accomplish this, we need to perform two separate trials. One uses a solid (powder) version of MgO, while the other uses Mg ribbon. With the results from these, we can use Hess’ Law to determine q=∆H. This provides both a safe and successful way of indirectly determining the heat of combustion for magnesium.

Magnesium will react with hydrochloric acid, because it is higher in the reactivity series than hydrogen. The magnesium displaces the hydrogen in the acid, so it forms magnesium chloride and hydrogen gas.

The purpose of this experiment is to verify the formula of magnesium oxide based on the masses of magnesium and the product (MgO). We verify the formula firstly by calculating the empirical formula of magnesium oxide and then calculating creating the magnesium oxide itself- a magnesium ribbon is combined with oxygen in the presence of air through combustion and this forms MgO. The empirical formula of a compound is the simplest method of expressing a chemical formula in whole-number ratios of the constituent atoms that are consistent with masses measured in the experiment; whereas the molecular formula expresses the chemical formula using the actual number of atoms. For example, the molecular formula of anthracene is C14H10 while the empirical formula is C7H5.

It is expected that the concentration of hydrochloric acid will increase the rate of the reaction between magnesium ribbon and hydrochloric acid. By increasing the concentration of

The ribbon is not. The crucible is heated for another 10 minutes. Step 9 is repeated until the ribbon become whitish. Then the crucible is allowed to cool.

Science Coursework – What factors effect the rate of reaction between magnesium and hydrochloric acid? Background Knowledge There are four factors that can affect the rate of reaction and they all rely on the collision theory. This is basically how hard and how often particles collide with each other. The more and harder they collide, the faster the reaction time will be.

When mixed with hydrochloric acid (appendix 4), they react violently, hence why only a small portion was allowed for this experiment. This supports the hypothesis, that is, it was predicted that such a reaction would occur as these metals are highly reactive, hence why the hydrogen gas produced was clearly visible (appendix 5). Tin is less reactive, however, according to the Metal Reactivity Series, reacts with acids at an extremely slow rate. This was evident in the experiment; however, more of a reaction would have occurred if the time frame was expanded. The metal was only left in the acid for five minutes; therefore, it had no reaction but could of, had it been left a while longer. Magnesium and Calcium are both alkaline earth metals which means that they all have an oxidation number of ‘+2’, making them highly reactive. Calcium is more reactive than Magnesium even though it is located below it on the periodic table (appendix 6) because its electron configuration is ‘2,8,8,2’ while Magnesium’s is ‘2,8,2’. This means that Calcium has more shells which, therefore, means that there is less of an attraction to the nucleus. This makes it easier for Calcium to lose electrons and react more so than Magnesium. According to the Metal Reactivity Series, in order from the most reactive to the least reactive, tin is located at around the middle of the

Kinetics of chemical reactions is how fast a reaction occurs and determining how the presence of reactants affects reaction rates. In this experiment the rate of reaction for Fe+3 and I- is determined. Because the rate of chemical reactions relates directly to concentration of reactants, the rate law is used to find the rate constant, and calculated with specified temperatures.

Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid