Essay: Chemical reactions

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  • Subject area(s): Science essays
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  • Published on: March 23, 2018
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The goal of the lab was to show learn about chemical reactions. It showed the different types of chemical reactions (synthesis, decomposition, single replacement, double replacement, and combustion.) In the lab different elements and compounds were combined to observe chemical reactions and see what they could look like. The reactions also showed whether or not predictions that were made were accurate or not. The reactions were observed to see what would happen before, during, and after the eight chemical reaction and to see what the chemical reactions could produce.


There are five types of chemical reactions: combustion, synthesis, decomposition, single replacement, and double replacement. To write an equation first it must be determined what type of reaction it is in order to predict the products accurately. Synthesis is the combination of two or three reactants into one single product. Decomposition is when one compound decomposes into two or more products. Single replacement is when there is a compound and an element and the element and a part of the compound are switched to for two different products. Double replacement is when there are two compounds and then the anions are switched to form two different compounds. Combustion is normally the reaction of a compound made up of hydrogen and carbon that reacts with oxygen to form water and carbon dioxide.

To begin to write the equation in ionic compounds the ions of each need to have a balanced charge. For example oxygen has a charge of -2 and sodium has a charge of +1 to make the charges equal the sodium must have a subscript of two to balance out the ions to equal zero. In reactions there is also the law of the conservation of mass. This law means that in chemical reactions there is the same amount of mass in the product as in the reactants whether it is in the form of a liquid, solid, or gas. To follow this law it is important to balance the equation. To do so coefficients have to be added on either side of the equation to make sure that there is an equal number of atoms of each element on either side of the equation. If it is an equation involving heat then there is a delta above the arrow to indicate that heat was added to create the reaction.

It is important to follow the safety rules in order to not get hurt or injured. It is important to wear goggles during the lab so that any liquids, gases, glasses, or extra materials doesn’t damage any eyes. It is also important to use hot mitts (whenever possible) to protect hands from potentially dangerous hot substances in order to prevent any burns and chemicals from landing on skin. It is also important to wear aprons whenever possible to prevent any damage to clothing or body from potentially dangerous chemicals, glass, or heat.


Reaction A

2Mg(s) + O2(g) -> 2MgO(s)

Reaction B

CaO(s) +H2O(l) -> Ca(OH)2(aq)

Reaction C

3CuSO4(aq) +2Na3PO4(aq)-> Cu3(PO4)2(aq) +3Na2SO4(s)

Reaction D

NaHCO3(s) -> Na(s) + H2O(l) + CO2(g)

Reaction E

2NaBr(aq) + Cl2(aq) -> 2NaCl(aq) +Br2(l)

Reaction F

Zn(s) + 2HCl(aq) -> ZnCl2(aq) +H2(g)

Reaction G

NaHCO3(aq) + HC2H3O2(aq) -> NaC2H3O2(aq) +H2O(l) +CO2(g)

Reaction H

CuSO4(aq) +Zn(s) -> ZnSO4(s) + Cu(aq)


Reaction A

Before: Silver, rectangular shape, malleable

During: white, bright, light

After: white, powdery, broken up/ashy

Reaction B

Before: White powder and water

During: Power dissolving into water

After: Milky white, non-transparent, dark blue ph strip of 11, slightly thick

Reaction C

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