Limiting Reactant Lab Report

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

Usually, the percent is a good amount less than 100 because of multiple factors including transfer between different lab tools and when an unfulfilled reaction takes place. In the case of this experiment, copper most likely was lost between transfers of the Copper (II) solution, although loss was attempted to be minimized. Also, after the reaction, the copper was filtered and some mass could have lost if the reaction was not fully carried out and all of the copper did not precipitate out of the solution. But, when the copper oxidized overnight on the heater, the reaction with oxygen added mass to the ending mass of copper. These areas of losing and gaining mass throughout the procedure equaled out in the end because the percent yield was very close to 100% as the actual yield was 0.7 grams of copper and the theoretical yield was 0.71 grams of copper. If the copper did not oxidize, it is believed that the percent yield would not have been as close to 100% as it was because the oxygen gave mass back that was lost along the way of 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 the experiment the magnesium reacts with the hydrochloric acid to create magnesium chloride and hydrogen. The balanced formula for this is:

Goal: To correctly identify what compound is formed and how close it is to the theoretical yield.

The purpose of the lab was definitely achieved, for by finding that the mole ratios of the theoretical and experimental were equivalent, it was able to reveal the relationship between the reactants and products of a chemical reaction. Since the ratios came out to be the same, it showed that the finding of the masses of substances and converting them to moles was done accurately and showed an understanding of how to perform those calculations. It was learned that with a given amount of a reactant, it is possible to predict what the amount of the product will be. It also showed that the relationship between the products and reactants showed that they were balanced. This information can be used in the real world when following recipes.

The term concentration refers to the amount of a substance present in a certain volume of liquid or gas. Increasing the concentration of the reactants will increase the rate of the reaction. If the concentration of a reactant in a solution is increased, there will be a greater number of particles in a given volume of solution. This means the particles are more likely to collide and therefore react when there are more of them. Collisions between particles are necessary for the reactants to rearrange and form the products. In this experiment, the rate of the reaction between magnesium ribbon and hydrochloric acid will be increased by adding a higher concentration of hydrochloric acid each time. The chemical equation between magnesium ribbon and hydrochloric acid can be written as:

In Chemistry, when a student conducts their experiment and is asked to calculate the percent yield for their reaction it may be possible that they can get either a low percentage yield or a high one even above 100%. The first thing they need to understand what a percent yield is to begin with. A percent yield is calculated to be the experimental yield divided by theoretical yield multiplied by 100, basically it is the total amount of product that could be created in a reaction, calculated referring to the beginning amount of the limiting reagent. The question here is if this is the result of a violation of the law of conservation of matter?

Your percent yield would be: 0.82044415 The balanced equation I came up with is 3CaCO3 + 2Li3N yields 3Li2CO3 + Ca3N2 as my answer.

During the experiment, 0.1400 g of Magnesium reacted with Oxygen (O2) in air to form .2300 g of Magnesium Oxide. The loosely spiral magnesium ribbon (approximately 16 cm) which had a shiny characteristic was turned into a dull grey powder after the reaction took place. The percent error for this experiment was 0.9453% error. This was found by calculating the following: ((Theoretical % - Experimental %) / Theoretical %) x 100. The error could have happened because since the reaction of Mg and O2 is so exothermic (temperatures above 1000 degree Celsius are obtained during the reaction), some Mg might have reacted with the N2 in the air (since the air contains 78% N2 and 21% O2) to create magnesium nitride (Mg3N2(s). The balance equation for this

In this today’s lab, Percent Yield of Hydrogen Gas from Magnesium and Hydrochloric Acid, the purpose is to study the stoichiometry of H2 produced from the reaction between magnesium (Mg) and hydrochloric acid (HCl). The chemical equation for this reaction is Mg +2HCl -> MgCl2 + H2. It was predicted that 0.0029 moles of hydrogen gas would be formed from 0.07g of magnesium metal and 10 mL of hydrochloric acid. The hypothesis was proven correct based on an actual yield of 0.00299 moles of hydrogen gas. We know this because after measuring the volume and pressure of our results, we used the Ideal Gas Law Equation to calculate the number of moles. We also calculated the percent yield by dividing the experimental number of moles of hydrogen gas

The magnesium was cut carefully at 2cm every time to ensure that no acid had more reactants

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

In a chemical experiment when two substances are reacting, one reactant will be consumed first then the other one and it will be call Limiting reactant. “The limiting reactant is a reactant in a chemical reaction that determines the amount of product produced” (Helmenstine). This is the substance that controls the results, depending on the amount that it can produce it’s going to be determinate how far the chemical reaction can go. The Percent Yield gives the amount of product that could possibly be produced in a given reaction. Percent yield measures how efficient the reaction is under certain conditions.” Percent yield measures how efficient the reaction is under certain conditions” (Boundless). To find the Percent Yield, we have to calculate

should be rewritten as “Add 0.5 g magnesium to 200 cm3 of 2M hydrochloric acid”