Mass is anything that takes up space. Mass is made up of small subatomic particles called atoms. Atoms have three main parts electrons, protons, and neutrons. The mass of the atom is found in the nucleus. The Law of Conservation of Mass states that mass cannot be created nor destroyed, and that the mass of the reactants will be equal to the mass of the products. This means that no matter what, the mass of the reactants when mixed together should be equal to their original masses. A chemical reaction changes one or more substances to be transformed into (a) new substance(s). A physical change is the change in somethings appearance. Chemical changes can be identified by its interaction with other substances. How does the mass of the substances …show more content…
The materials for the lab included: Sodium bicarbonate, acetic acid, large Erlenmeyer flask, balloon, small graduated cylinder, and an electric balance. The second step of the first experiment was to measure 10 mL of acetic acid in the graduated cylinder. Next, measure half a spoonful of sodium bicarbonate. To weigh the sodium bicarbonate it was placed in the flask and weighed, using the electronic balance. The weight of the sodium bicarbonate was recorded in a data table. After the sodium bicarbonate was weighed the acetic acid(inside the graduated cylinder) was weighed on the electric balance. The weight of the acetic acid was recorded in a data table as well. The acetic acid was then poured into the flask with the sodium bicarbonate. The balloon was used to quickly cover the opening of the flask, in order to prevent the gas from leaking. The product was weighed and compared to the weight of the …show more content…
This claim was made because it was backed up by our first experiment. Our first experiment showed that the products and the mass have the same mass. The four bars on the graph show the masses of the reactants and products of two experiments. In experiment 1 the mass of the reactants and products are very close to each other. The reactants have a larger mass because they had not created any gases that could escape. The graph proves the Law of Conservation of mass. The similar masses show that with less errors the experiment the products mass and the reactants mass will be equal. This investigation is tied into the Law of Conservation of Mass. The Law of Conservation of mass cannot be created or destroyed. This shows that after a chemical reaction none of the mass from the reactants can be destroyed and no more mass can be created. This evidence proves the Law of Conservation of
In our mini-lab yesterday, we put sugar cubes in a jar and shook them for three minutes. The first jar had one cube, the second had two cubes, and the third had three cubes. We were trying to find the impact of the shaking on the sugar cubes. Our sugar cubes represented the rocks, and the shaking was an outside force. My group’s hypothesis was that the sugar cubes would break up.
We had to mix baking soda, calcium chloride and water and then as a product we would have rocksalt and calcium carbonate, 2NaHCO₃+CaCl₂===>CaCO₃+CO₂+2NaCl+H₂O. We know that a chemical reaction took place because on the products into reactants equation the elements are equally transfered from one side to the other after the chemical reaction took place. We were given a plastic bag, that way we could do a closed experiment. We had to support that there were endothermic and exothermic reaction and that The Law of Conservation of Mass was present in this
Kinetic theory states that molecules are always in constant motion. Kinetic energy and molecule velocity increases as temperature increases. Reactions require collisions between reactant molecules or atoms. In chemical reactions, the reactants change into products when molecule collide with enough energy to break old bonds to make new ones. Collisions increase or become more violent between molecules at higher temperatures or decrease as the temperature is lowered.
Molar Relationships: What Are the Identities of the Unknown Compounds? The purpose of the experiment was to identify unknown compounds using knowledge on the concept of mole. The guiding question for this experiment is what are the identities of the unknown compounds? The numbers of moles and the identities of the compounds are the only given. To be able to identify the compounds the mass, molar mass and the number of moles will be needed.
Title: Exploring Reaction Rates Authors: Lauren Parker*, Serah Wiedenhoefer ( * - Primary Author)
Chemistry IA – Kinetic Experiments Practice Internal Assessment Investigating the relationship between KI concentration and its rate of reaction with H2O2, which is measured using a spectrophotometer. Research Question How will changing the concentration of KI affect its rate of reaction with hydrogen peroxide? Calculated as inverse of time taken for the blue-black coloration of tri-iodide ion and starch solution, measured using a spectrophotometer. Introduction:
Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated
can be a hazard to the students. Equipment and Materials the following equipment’s were required in the experiment: Equipment Reason for Choosing it 50 cm³ of HCL of varying concentrations I chose 50cm³ as a starting point, The different concentrations will be : 1.5, 1 and 2 M 0.06g of magnesium I chose 0.06 grams and it will have a length of 3 centimeters. Magnesium ribbon is an efficient way to check the rate of reaction. Pipette I am using a pipette to measure out the quantities for collecting the acid. I could have use a beaker or measuring cylinder to measure the volumes of acid and water, but chose a pipette because it's more accurate.
Then the balloon is lifted up so that the baking soda runs into bottle to react with the vinegar inside. Immediately the balloon is inflated by the carbon dioxide formed. The baking soda is kept constant when the experiment is repeated for another different amount of vinegar. Results/Findings When sodium bicarbonate and vinegar mix,
Research paragraph Jean-Marc de Villiers When Two Objects Collide Two moving objects, both possessing momentum by the product of their mass and velocity, collide with one another. Within the system created by their collision, there is a total momentum that is equal to their combined mass and the sum of their velocity.
Piaget’s experiment in figure 7.5 displays a child’s thought process concerning multiple layers of information. His experiment included showing a child two identical glasses of water. Both glasses appeared to be the same. The child concluded that the water was the same in both glasses. When a taller and thinner glass was utilized the child automatically proclaims that the new thinner glass has more water in it.
The Law of Multiple Proportions was proposed by John Dalton, a British schoolmaster and chemist, this law led to the Atomic theory in 1803. Dalton’s Atomic Theory was that all matter is made of atoms and they are indivisible and indestructible. He also believes that atoms of the same element can have different weights and atoms of different elements can have the same weight. Atoms are the smallest particles that take part in chemical reactions; and atoms do not always have to combine in simple
Dalton’s atomic theory contained the following ideas: All atoms of a given element are identical. The atoms of different elements vary in mass and size. Atoms are indestructible. Chemical reactions may result in their rearrangement, but not their creation or destruction. Dalton also outlined a law of multiple proportions, which described how reactants will combine in set ratios.
That caused a new initial reading of NaOH on the burette (see Table1 & 2). The drops were caused because the burette was not tightened enough at the bottom to avoid it from being hard to release the basic solution for titrating the acid. The volume of the acid used for each titration was 25ml. The volume of the solution was then calculated by subtracting the initial volume from the final volume. We then calculated the average volume at each temperature.
Introduction This module is all about Stoichiometry, composition and reaction. I chose this topic not because I am having a really hard time understanding it, but because I want to have a deeper understanding of the lesson. Before actually doing this, I watched some videos on YouTube in order to look for some techniques I can actually apply in doing some written works and execute as an example for this module. In this module, I will focus more on the different techniques on how to convert unit to unit that I learned from different sources and some I self-learned, and of course some from the discussion done by our teacher.