Chemical Reaction Lab Report

When combined Sodium Bicarbonate and Hydrochloric Acid, Carbon Dioxide is produced. The two chemicals do not undergo a change in color but a chemical change when CO2 is produced.

In this experiment, you have been asked by your teacher, to investigate the design of a small-scale airbag system they want to produce as a child safety device to put into baby strollers. Because of sodium azide’s toxicity (which is used in many vehicular airbags), it is suggested you use the reaction of NaHCO₃ (sodium bicarbonate or baking soda) with an aqueous solution of HCL (stomach acid) to produce CO₂ gas to test your engineering design. The reaction of hydrochloric acid and sodium bicarbonate is: HCL + NaHCO₃, one mole of CO₂ gas is produced. Regarding the other products, NaCl dissolves in the water to create a salt solution which occupies only a small portion of the volume inside the bag.

A chemical reaction is when substances (reactants) change into other substances (products). The five general types of chemical reactions are synthesis (also known as direct combination), decomposition, single replacement (also known as single displacement), double replacement (also known as double displacement), and combustion. In this lab, the five general types of chemical reactions were conducted and observations were taken before, during, and after the reaction. Then the reactants and observations were used to determine the products to form a balanced chemical equation. The purpose of this lab was to learn and answer the question: How can observations be used to determine the identity of substances produced in a chemical reaction?

The purpose of this experiment was to mix Alka-Seltzer with Hydrochloric acid in order to analyze Sodium Bicarbonate as an active ingredient in the Alka-Seltzer. The mixture will contain hydrochloric acid to only see the composition of Sodium Bicarbonate in the tablet once it reacts. The amount that reacted allowed us to determine how much of it is present in the tablet. The amount of sodium bicarbonate will be measure by using the ideal gas law PV=nRT. The experiment will be conducted in the lab, therefore we are going to use room temperature which ranges from 15 to 26 degrees celsius. At room temperature pressure ranges from 12.8 to 25.0 millimeters mercury according to its corresponding room temperature.In the ideal gas equation R is 0.08206latm/mol k which is a constant. Once we have those values we can calculates the number of moles that reacted in the mixture by solving for the missing value. With the number of moles we are able to find the mass in grams which is what will potentially tell us the composition of Sodium Bicarbonate in a tablet of Alka-Seltzer.

The objective of the experiment was to observe different reactions with different chemicals. The experiments emphasized on the chemical changes occurring in acids and bases as well as color changes and bubble formations. The experiments allowed for a better understanding of the undergoing chemical changes in mixtures. Some mixtures instantly changed colors while others were transparent or foggy. Some mixtures produced thick color that created solids called precipitates. Mixtures KI + Pb(NO3)2 and NaOH + AgNO3 both produce noticeable precipitates after a while. It was interesting to see the different acidic and base reactions like the fuchsia color formation in NaOH + phenolphthalein.

Discussion The purpose of this lab was to measure the mass of a solid reactant, in this case, NaHCO3, which is also known as baking soda, and to find the mass of the solid product NaCl (salt) as well. From there, the masses were to be converted into moles and created into ratios that showed the relationship between the reactants and products. That information was then compared to the theoretical data in order to check its accuracy and reveal the significance of mole ratios in chemical reactions.. During the experiment, hydrochloric acid (HCl) was added to the baking soda in order to begin the reaction.

From the results that were acquired from mixing the liquid reagents with each powder, it was determined that Unknown Mixture #1 consisted of baking soda and cornstarch. When individually testing the substances from Unknown Mixture #1 with the liquid reagents, a few noticeable reactions occurred. Mixing baking soda with vinegar caused bubbling to occur. This is because a neutralization reaction took place between the two reactants. In this reaction, sodium bicarbonate(baking soda) reacts with vinegar and produces sodium acetate, water, and carbon dioxide(HC2H3O2(aq) + NaHCO3(aq) NaC2H3O2(aq) + H2O(l) + CO2(g) ). The gaseous carbon dioxide most likely tried to escape into the atmosphere and caused the bubbling to occur. Another noticeable reaction

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

The mixing of vinegar and baking soda causes a chemical reaction. The mixture of baking soda and vinegar caused a chemical reaction, thus inflating the balloon. Five ml of baking soda and vinegar was added into the flask and balloon. The initial temperature is -25 °C. The final temperature is -23 °C.

Decompositions can have up to 4 potential ways it can be balanced in a chemical equations while only one equation can be correct. The purpose of this lab is meant to investigate which decomposition equation is correct. The guiding question for this experiment is “Which balanced chemical equation best represents the thermal decomposition of sodium bicarbonate?” given the equations NaHCO3 → NaOH(s)+CO2 (g), 2NaHCO3(s) → Na2CO3 +CO2(g)+H2O, 2NaHCO3 (s) → Na2O (s) + 2CO2 + H2O, NaHCO3 (s) → NaH (s) + CO (g) + O2 which will be denoted as hypothesis 1, 2, 3, and 4 respectively.

The main purpose of this lab was to use stoichiometry to determine the yield of NaCl based on a given amount of reactants. Stoichiometry is a method used in chemistry which utilizes the amounts of reactants, products and the coefficients of the balanced chemical equation, to determine measurements such as the excess and limiting reactants. The chemical equation for this lab was NaHCO3(s) + HCl(ag) NaCl(s) + H2O(l) + CO2(g) and in the end of the lab the H2O and CO2 were evaporated. The chemical equation was used to predict the amount of NaCl that should be produced from the the combination of NaHCO3(s) and HCl(ag). We observed two different chemical changes when the solution became cold in the beaker of NaHCO3(s) and HCl(ag) and when the solution began to bubble due to the production of CO2 gas. The limiting reactant was NaHCO3(s) because a set amount was used and the excess reactant was HCl(ag) because we were able to add the necessary amount needed to completely consume the amount of NaHCO3(s). After the bubbling stopped, we added 5 drops of HCl(ag) to prove that the reaction between the HCl and NaHCO3(s) had

Next, spatula tips of sodium bicarbonate were added to the solution until CO2 was no longer being produced. This was observed by when the solution stopped bubbling after the addition of the sodium bicarbonate. Once the sodium bicarbonate was no longer reacting with the

In conclusion, the chemical formula of the dehydrated sample was found to be CuCl2 and the formula for the hydrated sample was CuCl2 ·2H2O. Thorough experimental procedure was taken to obtain the water loss of the hydrated sample, therefore defining its chemical formula. As the hydrated sample of copper chloride changed colors throughout the heating process, a change in chemical composition was noted. The hydrate was originally a blue/green color, but as it was heated and lost its water, the hydrate turned brown. This chemical composition is known as the anhydrous residue.

Throughout the world, chemical reactions are taking place to either achieve a specific purpose or prevent a specific outcome. These reactions can be as simple as boiling water to pour a coffee in the morning or as complex as industrial level biochemistry. Whether you are aware of it or not, you create numerous amounts of chemical reactions every day. According to the collision theory, a chemical reaction will occur if two or more molecules collide with the right amount of energy and the right orientation. The energy that is required from the collision depends on the molecules and can be referred to as activation energy.