Introduction In this chemical reaction, the magnesium will dissolve in the hydrochloric acid to produce hydrogen gas. This is because magnesium is higher than hydrogen in the reactivity series. Therefore, when the two reactants are combined, a displacement reaction occus and the magnesium displaces the hydrogen, forming magnesium chloride and hydrogen gas. Mg (s) + 2HCl (aq) -> MgCl 2 (aq) + H 2 (g) Magnesium + Hydrochloric acid -> Magnesium Chloride + Hydrogen Aim The aim of this investigation is to observe the effect that the concentration of hydrochloric acid (independent variable) has on the rate of reaction (dependent variable) between the magnesium ribbon and the hydrochloric acid. …show more content…
If there is more surface area exposed to the hydrochloric acid, the particles of acid will have a greater area of magnesium to react with and form successful collisions, thus increasing the rate of reaction. - Volume of Hydrochloric Acid Used: An overall volume of 50ml of hydrochloric acid and water should be used for every trial. If a lesser volume is used, this will decrease the rate of reaction as there will be less particles in the HCl to collide with the Mg particles, which will lessen the chance for creating a successful collision, and thus lower the rate of the chemical reactions. - Timing of the experiment: Bung with delivery tube should be placed on the conical flask as soon as possible after the magnesium ribbon is dropped. This will ensure that as much of the hydrogen gas gets measured in the measuring cylinder above the trough, in order to obtain accurate measurements when calculating the rate of reactions. Stopwatch will begin as soon as the magnesium is dropped into the hydrochloric acid, so that the timing of the reaction is measured accurately. - Cleaning of the magnesium: The ribbon of magnesium will be cleaned with sandpaper to remove the coating on the magnesium metal caused by reactions with atmospheric gases. This needs to be done so that the measuring cylinder measures the gas produced from the reaction
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)
In the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The balanced formula for this is:
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
An experiment was carried out to predict the limiting reactant in a chemical reaction between Magnesium and Hydrochloric acid, using the mole concept.
In analysis of the graphs created from the magnesium’s reaction pressure released over time, it appears that we may have had a possible source of error. According to our T.A., the powder should have a faster rate of reaction due to its surface area. However, in our experiment, the reaction rates were found to be similar due to the closeness of the slopes. For the first reaction (trial) of each magnesium type, we had used 0.2 grams due to a communication error. For the second reaction (trial) of each magnesium type, we used 0.02 grams. Despite the mass differences, the slopes were very close to one another but with the ribbon reactions appearing to be faster due to their slightly larger slopes. The ribbon reactions were shown to have a slope in
In the second reaction, when the magnesium ribbon is heated, it undergoes the reaction, 2Mg(s) + O₂(g) → 2MgO(s). The magnesium reacted with oxygen in the air to form magnesium oxide when the magnesium ribbon was heated and it produced a white, matte, and crumbly product. This indicates that the the product formed is magnesium oxide, a dull, white, substance. The reaction is classified as a synthesis reaction because the magnesium and oxygen combined to form one product.
Engage: The teacher will prepare beforehand the two plastic cup solutions. The teacher will pour 100mL of water in one clear plastic cup and add 10g of magnesium sulfate. Stir until the solution is clear. The teacher will pour 50 mL of water in another clear plastic sup and add 5 g of sodium carbonate. Stir until the solution is clear. The teacher will hold up the two clear colorless solutions and slowly pour the smaller amount into the larger. Students will record their observations and questions they have about the reaction in their Science Interactive Journals.
Equation of magnesium and hydrochloric acid: 2 HCl+ + Mg [IMAGE]Mg2+ + H2 Measuring rates of reaction In this investigation there are two experiments that can be used to test rates of reaction. Using a gas syringe As more gas is produced the plunger inside the syringe moves out of the syringe so the gas can be measured by marks on the syringes length.
The goal of this experiment was to determine the rate law for the reaction between magnesium metal and hydrochloric acid. In order to find the overall rate law of this reaction, the total pressure change of the reaction is recorded which allows the rate to be determined by evaluating the slope of the line pressure versus time before the reaction reaches completion. This technique is using pressure as a function of time. The equation that will be used to calculate the pressure of the hydrogen gas that is produced in the reaction is the ideal gas law or PV=nRT. The reaction that is used in this study between magnesium shot and hydrochloric acid is: Mg(s) + 2H+(aq) + Mg2+(aq) + H2(g). The theoretical rate law for this reaction that was expected
Overall, the results were almost as expected. It was predicted that Magnesium and Calcium would have a similar reaction will the hydrochloric acid and produce approximately that same quantity of hydrogen gas. However, the results demonstrated that the Calcium reacted more vigorously than expected and produced a larger quantity of hydrogen gas. The reaction which occurred whilst using Magnesium resulted exactly like the prediction. It was expected that the metal would bubble, eventually dissolve and produce gas which would potentially displace the water in the test tube. With the reaction involving Calcium, it was not predicted that it would heat up the conical flask and react as violently. It was expected that the Tin would either have a
The reaction used to produce hydrogen is : Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g). The reaction is carried out with excess hydrochloric acid, therefore the volume of hydrogen gas produced would depend on
Dependent variables: We used time in minutes and seconds for Hydrochloric acid to break down and dissolve the magnesium ribbon in till it’s gone.
Since copper is below hydrogen in the activity series, the copper will not replace the hydrogen to form with the chlorine, therefore the single reaction will not occur and there will be no reaction. Copper wire will not have any effect on the experiment since it does not react with hydrochloric acid, which makes it perfect to use as the basket to hold the magnesium in place.
Experiment to investigate factors affecting the rate of reaction between magnesium ribbon and hydrochloric acid