Chemical Reactivity Lab Report

The main objective of this experiment is to differentiate between a physical change and a chemical change.

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?

Ammonium nitrate (NH4NO3), is classified as a salt. The salt family of chemicals contains ions, which are particles with electrical charges. Due to the fact that opposite polarity ions attract each other, they form a solid crystal that is called salt. This when seen by the naked eye seem like a simple reaction. Bu, in reality this occurs in two different steps and each step a change of energy takes place.

Dichloromethane has a molar mass of 84.93 g/mol. It has a density of 1.325 g/mL at 25°C and a boiling point of 39.8-40.0°C. Dichloromethane is an irritant, a carcinogen, and highly toxic.

When the zinc was dropped in the hydrochloric acid, the substance began bubbling vigorously, forming a precipitate. Eventually, the zinc dissolved completely. After the lit wooden splint broke the surface of the test tube, there was a loud popping noise. The gas that was released was hydrogen from the acid and the popping noise was a result of the Hydrogen being burned up by the fire creating a small explosion. Two chemical changes occurred in this test: one with the formation of a precipitate (a textbook sign of a chemical change), and the other when the explosion

Experiment 2 focused on finding the enthalpy of solution of magnesium chloride. Testing the enthalpy of solution started with measuring out 10 mL of deionized water in a graduated cylinder for three separate trials, each trial having a different mass of magnesium chloride. The water was then poured into a well of a Styrofoam calorimeter then the initial temperature of water was taken using a temperature probe and the LoggerPro programming. A measured amount of magnesium chloride was placed in the same well as the water in the calorimeter,

6. The mass number is equal to an atom’s number of protons and neutrons added together.

Purpose: The purpose of this experiment is to observe a variety of chemical reactions and to identify patterns in the conversion of reactants into products.

10) When HCl was added, the H⁺ ions reacted with the NH₃ to form NH₄⁺. This causes the [NH₃] to

If all atoms want to have 8 electrons on their outer shell, what should happen between Ca and S for each atom to reach that state of having 8 valence

7. The more-electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion.

In part 1, the precipitate that forms is a aluminum hydroxide and in part 2 it is magnesium hydroxide. A precipitate is an insoluble solid that emerges from a liquid solution. When the emergence of the insoluble solid from solution happens, it is called precipitation. The property change in the reactants of the lab are when the water, alum, ammonia, react and create the aluminum hydroxide. When the precipitate is formed, it is an endothermic reaction because the change in the product, aluminum hydroxide, decreases in temperature. This is a chemical reaction because different elements rearrange themselves to form a new substance and while they do so, they either absorb heat or give it

This reaction occurred through a physical change through a reaction with the pressure and temperature of the water and gas in the

Fatima Gowher Uzma Gowher Tanishq Gadkari Fritz Flores Block 1 Chemistry Honors AbstractWhat happens when two merely different “things” are combined? By things, I mean two different substances.

Zumdahl and Donald J. DeCoste (Introductory Chemistry: A Foundation), two ionic compounds are placed in water and react and form two new compounds. There is evidence of a double-replacement reaction when a precipitate will form when a reaction occurs. There could also be a change in color, temperature, and possibly gaseous productions. Most commonly, there will be a color change and formation of a precipitate. During this lab, many chemicals will be involved that are not meant to contact skin or eyes. They can burn, sting, or irritate the skin. In order to prevent this, we must wear safety goggles throughout the entire procedure and be careful while dealing with the chemicals. We also need to be responsible and not touch, smell, or taste the chemicals at any point within this lab. The chemical formulas of the aqueous solutions of ionic compounds in this lab that are used are KNO3 (Potassium Nitrate), Mg(NO3)2 (Magnesium Nitrate), Fe(NO3)3 (Iron (III) Nitrate), Zn(NO3)3 (Zinc Nitrate), 3Cu(NO3)3 (Copper Nitrate), Ca(NO3)2 (Calcium Nitrate), K3Fe(CN)6 (Potassium Ferricyanide), Na3PO4 (Sodium Phosphate), Na2SO4 (Sodium Sulfate), NaOH (Sodium Hydroxide), NaCl (Sodium Chloride), and Na2CO3 (Sodium Carbonate). These are all categorized as aqueous based on the general solubility