Maalox Lab Report

One change that demonstrates a positive test in this lab is precipitate forming. If silver nitrate solution is mixed with a substance and a precipitate forms, chloride ions must be present in that substance. Another change the demonstrates a positive test in this lab is a colour change to a dark red colour. If potassium thiocyanate is mixed with a substance and the colour of the substance changes to dark red, Iron (III) ions must be present in the substance. Why do you think chemical tests, similar to tests used in this investigation are called

The purpose of doing a lab based on endothermic and exothermic reaction is to tell which is an endothermic reaction or which is an exothermic reaction like baking soda and calcium chloride. The lab setup for this lab are, five grams of baking soda, five grams of calcium chloride, one plastic bag, 30 ml of water, a 50 ml beaker, a rubber band, and two thermometers. During the experiment we found out about all the responding variables we had. For example, calcium chloride and water responded together making its side of the bag warm. Also with the water and baking soda, when the collided together it made there side of the bag cold.

The formation of a new substance is the result of the chemical changes that the reactants undergo. The manganese and hydrochloric acid will both experience chemical changes in order

When elements or compounds react with each other, under the right circumstances, a chemical reaction may occur, forming a new product. According to www.rico.edu, “A chemical reaction is the change of a substance into a new one that has a different chemical identity.” However, how is it possible to see whether such reaction has actually occurred? There are various indications of when a chemical reaction has occurred. For example, such indicators include a change in color, a noticeable odor once the reaction is completed, the formation of precipitate or of bubbles, the production of gas, or the transfer of energy which can shown by a change or release of either heat or light. Such examples are accurate signs of when a chemical reaction has, in fact, occurred.

We already knew that exothermic means to exit or release heat energy. Endothermic means to absorb heat energy. Chemical reactions are when one thing changes into another but it cannot return to it’s original form. We read about instant hot packs and cold packs and how they are chemical reactions. When water mixes with different salt or some substances it can cause a decrease or increase in temperature. In our experiment our guiding question was which of the following substances would make an economical hot pack or cold pack? This goes to show how you can use your background information on endothermic and exothermic also chemical reactions to make and economical cold pack or hot pack you would have to think through what substance would work

An Exothermic reaction releases heat which causes the temperature of the surroundings to increase. An endothermic reaction absorbs heat and cools the surrounding. (UC DAVIS CHEM WIKI organisation, 2015) W Reactants in exothermic reactions covert chemical energy to heat energy which causes the temperature to rise. Reactants gain energy in the endothermic process which comes from the substances used in the reaction and the reaction gets cold. Eventually, heat is absorbed from the surroundings and the mixture returns to room temperature. These reactions can be divided by chemical reaction and physical reaction. Chemical reactions are chemicals or substances which change to one or more other substances. While, physical reaction includes a change

The purpose of this lab experiment is to understand the difference between physical and chemical change and determine if these experiments are physical or chemical changes. A physical change is one that does not alter the identifying properties of a substance. A chemical change is one that produces a new substance with new properties. Hypothesis: Dissolving 2 g of sodium chloride in 50 ml of water will cause a physical change; Evaporating the sodium solution is a physical change; Burning the nichrome wire is a physical change; Burning the magnesium ribbon is a chemical change; Mixing silver nitrate and hydrochloric acid is a chemical change; Putting silver chloride filtrate in the sunlight is a physical change; Putting the aluminum

This experiment can create an endo and exothermic reaction. “The endothermic reaction means that the temperature drops, but it will drop slowly”. An endothermic reaction happens when energy is used to break all of the reactants and break away from every single particle in the substance causing the temperature to drop. An exothermic reaction is when the temperature rises and just like the endothermic reaction it will rise slowly. An exothermic reaction is very similar to an endothermic reaction, but

The first and third reactions are categorized as endothermic because there was a decrease in temperature, resulting in a cooler temperature. In reactions one and three, heat flowed from the surroundings and into the system, which left the reaction to seem like it was being cooled. The second and fourth reactions are categorized as exothermic because there was an increase in temperature, resulting in a warmer temperature. In reactions two and four, heat escaped from the system and was absorbed by the surroundings, which left the reaction to seem like it was heating up. Endothermic reactions occur when the system absorbs heat from its surroundings. Exothermic reactions occur when the system releases heat into the surrounding. Without the subject of thermochemistry, endothermic and exothermic reactions may be unheard

An exothermic reaction is a chemical reaction that releases energy by light or heat. It is the opposite of an endothermic reaction. An exothermic reaction will occur spontaneously, while and endothermic reaction needs energy to occur.

Exothermic reactions occur when the forming of a chemical bond releases energy therefore creating an exothermic process (Kentchemistry.com, 2015). An exothermic reaction has a negative deltaH, because the enthalpy of the products is lower than the enthalpy of the reactants of the system (Chemwiki.ucdavis.edu, 2015). An Endothermic reaction absorbs energy in the form of heat. In an endothermic reaction deltaH is positive because the enthalpy of the products is higher than the enthalpy of the reactants in the system (Chemwiki.ucdavis.edu, 2015).

An endothermic reaction is when more energy is absorbed than released and an exothermic reaction is when more energy is released than absorbed. The change in enthalpy that is associated with the mix of solution is called the heat of

Heat of formation measures the theoretical amount of energy released in reaction. (Helmenstine, 2014) It is calculated using the formula on the screen. Heat of combustion measures the experimental amount of energy released in a reaction. (Oliver, 2014) It can be calculated using the formula on the screen.

Observations of imploding thin-shell capsules have demonstrated an increasing discrepancy between predictions from single fluid hydrodynamic simulations and experimentally measured fusion yield as the Knudsen number (mean-free-path over system size) is increased. (-- removed HTML --) (-- removed HTML --) 1,2 (-- removed HTML --) (-- removed HTML --) The sensitive dependence on the Knudsen number indicates that these discrepancies may be due to a breakdown of single fluid hydrodynamics and thus motivates the need for multifluid (-- removed HTML --) (-- removed HTML --) 3,4 (-- removed HTML --) (-- removed HTML --) or kinetic modeling. (-- removed HTML --) (-- removed HTML --) 5,6 (-- removed HTML --) (-- removed HTML --) Specific

An exothermic reaction is one in which there is a release of energy (usually heat) from the system (Ashworth & Little, 2001). In other words, the energy of the system decreases, and thus H is negative. Because heat is being transferred out of the system (i.e., the reaction requires no external energy source), exothermic reactions are self-sustaining (Ashworth & Little, 2001). Notable examples of exothermic reactions include combustion reactions, where oxygen (O2) reacts with another substance, usually to form carbon dioxide and water (CO2 + H2O) (Kung & Lerner, 2014). Combustion can be seen in many facets of everyday life, from wood fires to the engines of many vehicles (the combustion of gasoline has the following chemical equation: 2C8H18 + 25O2 + 2N2 12CO2 + 4CO + 4NO + 18H2O + heat—this illustrates the convention of placing “heat” in a chemical equation, which, if listed as a product, is an indicator of an exothermic reaction; this equation is also an example of incomplete combustion, since an ideal combustion reaction would have no products save carbon dioxide and water; often, the oxygen fueling a combustion reaction is consumed before complete combustion can occur (Lew, 2015)). On a smaller scale, exothermic reactions can be used to create heating devices such as hand warmers, which can be calibrated (by analyzing the change in heat of the chemicals involved in the device) to produce an optimal amount of heat. [SOME MORE]