Alkenes and Alkynes have similar naming rule as with Alkanes. Alkenes are hydrocarbons with one or more double bonds. There is one special property by Alkenes, some molecules have same structure but different geometry are called Geometric Isomers. There're mainly 2 types of isomers, cis and trans.
Alkynes are hydrocarbons with one or more triple bonds, their general formula is Cn H2n-2, they have similar naming rules to alkenes except they do not have geometric isomers.
Here is a link to show you what Alkenes and Alkynes really are:
http://www.youtube.com/watch?v=7XbYhjyUI-M
Monday, May 30, 2011
Monday, April 4, 2011
Percent Yield
So today we did some stuff about percent yield. It is a ratio of amount of product obtained to amount of product expect. Let's simplify it, which is the grams of product recovered divided by the grams of product expected from stoichiometry. Then multiply the results by 100%. We also did something called percent purity, it is the ratio of mass of pure substance to mass of impure expressed in a percent. Which is mass of pure substance divided by mass of impure substance and multiply the results by 100%.
http://www.youtube.com/watch?v=TKNxdL7DN1I
http://www.youtube.com/watch?v=TKNxdL7DN1I
Tuesday, March 15, 2011
Lab 6D
So today we did a lab which is determining the limiting reactant and percent yield in a precipitation reaction. The objectives are to observe the reaction between solutions of sodium carbonate and calcium chloride; To determine which of the reactants is the limiting reactant and which is the excess reactant; to determine the theoretical mass of precipitate that should form and to compare the actual mass with the theoretical mass of precipitate and calculate the percent yield.
Monday, March 7, 2011
Stoichiometry Exercise
Is a branch of chemistry that deals with the quantitative relationships that exist between the reactants and products in chemical reactions. In a balanced chemical reaction, the relations among quantities of reactants and products typically form a ratio of whole numbers. For example, in a reaction that forms ammonia (NH3), exactly one molecule of nitrogen (N2) reacts withc) three molecules of hydrogen (H2) to produce two molecules of NH3:
- N2 + 3H2 → 2NH3
Example 1 : Ca(s) + 2HCl(aq) ----> CaCl2(aq) + H2(g)
a) How many atoms of Ca are needed to produce 1 molecule og Hydrogen?
Ans : Base on the equation : 1 mole of Ca/1 mole of Hydrogen = 1
Ans : Base on the equation : 1 mole of Ca/1 mole of Hydrogen = 1
b) How many moles of HCl are needed to produce 0.452 moles of CaCl2?
Ans : 0.452Ca x 2 moles of HCl/1 mole of Ca = 0.904mol
c) How many grams of Ca will react with 1.05moles of HCl?
Ans : 1.05moles of HCl x 1mole of Ca/2Hcl = 0.525moles of Ca
d) How many grams of CaCl2 will be formed when 2.00g of hydrogen is formed?
Ans : 2.00g/2 moles of H2 x 1 mole of CaCl2/1 mole of H x (40.1 + 35.5 x 2)g = 111.1gCaCl2
e) How many moles of of HCl are needed to form 6.12grams of CaCl2?
Ans : 6.12g of CaCl2/(40.1 + 35.5 x 2)mol of CaCl2 x 2 moles of HCl/1 mole of CaCl2 = 0.11 mol of HCl
Tuesday, March 1, 2011
Chapter 6 - Stoichiometry
As the definition above, Stoichiometry deals with quantitative analysis of chemical reactions, it is also the relationship between reactants used and products produced. It can use as molecules AND moles; it can also be used as conversion factors. The coefficient in balanced equations tell us the number of moles reacted or produced.
Stoichiometry calculations can predict how elements and components diluted in a standard solution react in experimental conditions. Stoichiometry is founded on the law of conservation of mass: the mass of the reactants equals the mass of the products.
A stoichiometric amount or stoichiometric ratio of a reagent is the amount or ratio where, assuming that the reaction proceeds to completion:
- all reagent is consumed,
- there is no shortfall of reagent, and
- no residues remain.
Here is a little video that i found on youtube that could help you understand more about Stoichiometry - http://www.youtube.com/watch?v=rESzyhPOJ7I
Thursday, February 24, 2011
Exothermic And Endothermic Reaction
An exothermic reaction is a chemical reaction that
An endothermic reaction is a chemical reaction that
Some examples of endothermic processes are:[2]
Expressed in a chemical equation:
- reactants → products + energy
Examples of exothermic reactions
- Combustion reactions of fuels
- Neutralization reactions such as direct reaction of acid and base
- Adding concentrated acid to water
- Burning of a substance
- Adding water to anhydrous copper(II) sulfate
- The thermitereaction
- Reactions taking place in a self-heating can based on lime and aluminum
- The setting of cementand concrete
- Many corrosion reactions such as oxidation of metals
- Most polymerisation reactions
- The Haber-Bosch process of ammonia production
Expressed in a chemical equation:
- reactants + energy → products
For an endothermic reaction, this gives a positive value for ΔH, since a larger value (the energy absorbed in the reaction) is subtracted from a smaller value (the energy used for the reaction).
- A chemical cold pack consisting primarily of ammonium nitrate and water.
- Evaporation of water
- Photosynthesis
Monday, February 21, 2011
Enthalpy Calculations
So today we did some notes on enthalpy calculations. It is a measure of the total energy of a thermodynamics system. It includes the internal energy. Which is the energy required to create a system, and the amount of energy required to make room for it by displacing its environment and establishing its volume and pressure. Delta H is the energy change in the reaction in the kJ/mole. The enthalpy of a system is defined as: H= U + pV
This is a video that will help u understand how to calculate Delta H in some enthalpy problems: http://www.youtube.com/watch?v=NoRg7eGfb9k
This is a video that will help u understand how to calculate Delta H in some enthalpy problems: http://www.youtube.com/watch?v=NoRg7eGfb9k
Monday, February 7, 2011
Types of Chemical Reactions
So last day we did a lab on types of chemical reactions, the types of reaction we did were synthesis, decomposition, single replacement and double replacement. So the purpose of the lab was just to observe how different chemical reactions work. We don't really have much trouble during the lab because the procedures were well written.
I also found a link which could help us all to know more about the types of chemical reactions
http://www.youtube.com/watch?v=tE4668aarck
I also found a link which could help us all to know more about the types of chemical reactions
http://www.youtube.com/watch?v=tE4668aarck
Tuesday, January 25, 2011
Balancing Equation
Today we are gong to talk about how to make the number of atoms of each kind on the relevant side equal to those on the product side
Here are some rules :
1. balance the atoms which only occur in one molecule on each side
2. balance the whole group
3. dont jump all over an equation
4. in an elemental form
Examples~
1. Al + CuCl2 ----> Al2Cl3 + Cu
step 1 : (4)Al + (3)CuCl2 -----> (2)Al2Cl3 + (3)Cu
step 2 : u should check if the molecules on both sides are equal
(4Al , 3Cu, 6Cl = 4Al , 3Cu, 6Cl)
2. KOH + H3PO4 -----> K3PO4 + H2O
step 1 : (3)KOH + H3PO4 ----> K3PO4 + (3)H2O
step 2 : checking
(3K, 7O, 6H, 1P = 3K, 7O, 6H, 1P)
Here are some rules :
1. balance the atoms which only occur in one molecule on each side
2. balance the whole group
3. dont jump all over an equation
4. in an elemental form
Examples~
1. Al + CuCl2 ----> Al2Cl3 + Cu
step 1 : (4)Al + (3)CuCl2 -----> (2)Al2Cl3 + (3)Cu
step 2 : u should check if the molecules on both sides are equal
(4Al , 3Cu, 6Cl = 4Al , 3Cu, 6Cl)
2. KOH + H3PO4 -----> K3PO4 + H2O
step 1 : (3)KOH + H3PO4 ----> K3PO4 + (3)H2O
step 2 : checking
(3K, 7O, 6H, 1P = 3K, 7O, 6H, 1P)
Monday, January 10, 2011
Diluting Solutions to Prepare Workable Solutions
We should make solutions of any concentrration from a more concentrated source.
We can make it by a simple equation.
M1V1 = M2V2
Example 1 :
Theres a 40.0mL of 0.400M NaOH solution is diluted to a final volume of 200.0mL, calculate the new concentration.
Let x be the new concentration.
0.400 x 40.0/1000.0 = 100/1000x
x= 6.25
The new concentration is 6.25M
Example 2 :
A 0.700M solution is concentrated by evaporation to a reduced final volume of 200.0mL and a molarity of 1.65M. Calculate the original volume.
Let V be the original volume.
0.700V = 200/1000 x 1.65
V = 2.33
The original volume was 2.33L
The original volume was 2.33L
Wednesday, January 5, 2011
Molar Concentration/ "Molarity" Conversation
Molarity is a number of moles of solute in 1 L of solution. We use "M" to denote molar concentration and ift has the units of "moles/L"
E.g. A 100 M solution is MORE concentrated than a 5 M solution.
Formula: Molarity = moles of solute(mol)/ volume of solution(L) aka M = mol/L
We also learned how to calculate the volume. We will learn more about this topic next class
E.g. A 100 M solution is MORE concentrated than a 5 M solution.
Formula: Molarity = moles of solute(mol)/ volume of solution(L) aka M = mol/L
We also learned how to calculate the volume. We will learn more about this topic next class
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