The document contains examples of various types of chemical reactions:
a) Combustion reactions of hydrocarbons and alcohols reacting with oxygen.
b) Decomposition reactions of ammonium nitrate decomposing.
c) Combination reactions of nitrogen and hydrogen forming ammonia, and potassium oxide reacting with water.
d) Stoichiometric calculations involving moles, masses, and molecules in several chemical equations.
This powerpoint talks about the law Conservation of Mass. You will know who,when and how the discoverer found the Law of Conservation of mass. This is a work that is very good, because it has lots of images, example and you will undestand everything because the vocabulary is simple and anyone can understand it
A World of Regions - The Contemporary WorldtitserRex
This presentation was made to help other teachers in TCW discussed the topic more meaningful.
-from the book "The Contemporary World " by L. Claudio and P. Abinales
Hi Chers!
Just wanna help you guys since March 2020 LET was Cancelled here's a powerpint reviewer for Gen. Ed. - Mathematics.
Hope It will help you.
just click the link and download the Document.
Good Luck and Always Pray. I Know Papasa Kayo!
https://dollarupload.com/dl/91446
This powerpoint talks about the law Conservation of Mass. You will know who,when and how the discoverer found the Law of Conservation of mass. This is a work that is very good, because it has lots of images, example and you will undestand everything because the vocabulary is simple and anyone can understand it
A World of Regions - The Contemporary WorldtitserRex
This presentation was made to help other teachers in TCW discussed the topic more meaningful.
-from the book "The Contemporary World " by L. Claudio and P. Abinales
Hi Chers!
Just wanna help you guys since March 2020 LET was Cancelled here's a powerpint reviewer for Gen. Ed. - Mathematics.
Hope It will help you.
just click the link and download the Document.
Good Luck and Always Pray. I Know Papasa Kayo!
https://dollarupload.com/dl/91446
This PowerPoint covers Stoichiometry and the concept of the Mole for my CHEM 2800 class that teaches elementary education majors the basics of chemistry
Balancing Chemical Equation. A chemical equation shows the starting compound(s)—the reactants—on the left and the final compound(s)—the products—on the right, separated by an arrow. In a balanced chemical equation, the numbers of atoms of each element and the total charge are the same on both sides of the equation.Each substance is specified by its chemical formula, optionally preceded by a number called stoichiometric coefficient. The coefficient specifies how many entities (e.g. molecules) of that substance are involved in the reaction on a molecular basis. If not written explicitly, the coefficient is equal to 1. Multiple substances on any side of the equation are separated from each other by a plus sign. The standard notation for chemical equations only permits all reactants on one side, all products on the other, and all stoichiometric coefficients positive. A chemical equation is the symbolic representation of a chemical reaction in the form of symbols and chemical formulas. The reactant entities are given on the left-hand side and the product entities are on the right-hand side with a plus sign between the entities in both the reactants and the products, and an arrow that points towards the products to show the direction of the reaction. The chemical formulas may be symbolic, structural (pictorial diagrams), or intermixed. The coefficients next to the symbols and formulas of entities are the absolute values of the stoichiometric numbers. The first chemical equation was diagrammed by Jean Beguin in 1615.
In the symbolic equation, chemical formulas are used instead of chemical names for reactants and products, while symbols are used to indicate the phase of each substance. It should be apparent that the chemical shorthand method is the quickest and clearest method for writing chemical equations.
n a chemical change, new substances are formed. In order for this to occur, the chemical bonds of the substances break, and the atoms that compose them separate and rearrange themselves into new substances with new chemical bonds. When this process occurs, we call it a chemical reaction. A chemical reaction is the process in which one or more substances are changed into one or more new substances.
Reactants and Products
To describe a chemical reaction, we need to indicate what substances are present at the beginning and what substances are present at the end. The substances that are present at the beginning are called reactants and the substances present at the end are called products.
Sometimes when reactants are put into a reaction vessel, a reaction will take place to produce products. Reactants are the starting materials, that is, whatever we have as our initial ingredients. The products are just that—what is produced—or the result of what happens to the reactants when we put them together in the reaction vessel. If we think about baking chocolate chip cookies, our reactants would be flour, butter, sugar, vanilla, baking soda, salt and chocola
2. 3.34
a) Mass of 5.50x10-3 moles of CdS
Cd 112
144 gCdS
S 32 5.76 x10 −3 molCdS * = 0.829 gCdS
molCdS
144
b) Moles of NH4Cl in 112.6g
N 14
H1x4=4
Cl 35.5
53.5
1molNH 4Cl
112.6 gNH 4Cl * = 2.10 gNH 4Cl
53.5 gnH 4Cl
c) Molecules in 1.305 x 10-2 moles of C6H6
−2 6.02 *10 23 molecules
1.305 *10 molC6 H 6 * = 7.86 *10 23 molecules
mol
d) Oxygen atoms in 4.88 x 10-3 mol Al(NO3)
−3 6.02 *10 23 molecules 9 O atoms
4.88 *10 molAl ( NO3 ) 3 * * = 2.64 *10 23 O atoms
mol molecule
3. 3.58 C6H12O6 2C2H5OH + 2CO2
2 mol CO 2
a) 0.400 mol EtOH * = 0.800 mol CO 2
1 mol EtOH
b)
Molecule C6H12O6 C2H5OH CO2
C 12 6 72 C 12 6 24 C 12 1 12
O 16 6 96 O 16 1 16 O 16 2 32
H 1 12 12 H 1 6 6
Total 18 45 44
0
1 mol EtOH 1 mol glucose 180 g glucose
7.5 g EtOH * * * = 15 g glucose
45 g EtOH 2 mol EtOH 1 mol glucose
c)
1 mol EtOH 2 mol CO 2 44 g CO 2
7.5 g EtOH * * * = 7.3 g glucose
45 g EtOH 2 mol EtOH 1 mol CO 2
4. 3.60
a) Balance: Fe2O3 + CO Fe + CO2
Fe2O3 + 3CO 2Fe + 3CO2
b)
1000g 1 mol Fe 2 O 3 3 mol CO 28 g CO
0.150 Kg Fe 2 O 3 * * * * = 78.95 g CO
1 Kg 159.6 g Fe 2 O 3 1 mol Fe 2 O 3 mol CO
c)
grams Fe:
1000g 1 mol Fe 2 O 3 2 mol Fe 55.8 g Fe
0.150 Kg Fe 2 O 3 * * * * = 104.9 g Fe
1 Kg 159.6 g Fe 2 O 3 1 mol Fe 2 O 3 mol Fe
grams CO2
1000g 1 mol Fe 2 O 3 3 mol CO 2 44 g CO 2
0.150 Kg Fe 2 O 3 * * * * = 124.0 g CO 2
1 Kg 159.6 g Fe 2 O 3 1 mol Fe 2 O 3 mol CO 2
d)
Fe2O3 + 3CO 2Fe + 3CO2
150g + 78.9g = 104.9g +124g
228.9g = 228.9 g