Synthesis/Decomposition Reactions
... In these reactions, two different molecules or atoms combine to form a single substance. ...
... In these reactions, two different molecules or atoms combine to form a single substance. ...
Introduction to Chemistry
... Evidence of Chemical Change EPOCH is an acronym that stands for evidence that a chemical reaction has occurred. ...
... Evidence of Chemical Change EPOCH is an acronym that stands for evidence that a chemical reaction has occurred. ...
Unit 5 Practice Problems (with answers at end) - H
... 7. To produce the original "water gas" mixture, carbon (in a combustible form known as coke) is reacted with steam: ...
... 7. To produce the original "water gas" mixture, carbon (in a combustible form known as coke) is reacted with steam: ...
Reactions Unit Plan
... 1. Classify the type of chemical reaction as synthesis, decomposition, single replacement, double replacement, and combustion. 2. Predict the products of a chemical reaction using the activity series of metals and solubility rules. B. Apply the Law of Conservation of Mass to writing and balancing ch ...
... 1. Classify the type of chemical reaction as synthesis, decomposition, single replacement, double replacement, and combustion. 2. Predict the products of a chemical reaction using the activity series of metals and solubility rules. B. Apply the Law of Conservation of Mass to writing and balancing ch ...
CHEMICAL REACTIONS Chapter 4
... 2. How many moles of hydrogen gas are produced? 3.How many moles of ZnCl2 are ...
... 2. How many moles of hydrogen gas are produced? 3.How many moles of ZnCl2 are ...
Chapter 6 Chemical Reactions and Change
... A chemical equation gives the chemical formulas of the reactants on the left of the arrow and the products on the right. Since matter in a chemical reaction is conserved, the number of atoms you begin with must equal the number oand type you end up with. ...
... A chemical equation gives the chemical formulas of the reactants on the left of the arrow and the products on the right. Since matter in a chemical reaction is conserved, the number of atoms you begin with must equal the number oand type you end up with. ...
Zumdahl`s Chap. 4 - The University of Texas at Dallas
... Weak Electrolytes are mostly molecular. ...
... Weak Electrolytes are mostly molecular. ...
Double Replacement Reactions
... First, if the equation is not complete, write out the correct formulas… 1. Use charges 2. Know the 7 Diatomic Elements: Make sure you know which elements are diatomic so you can write the correct equation. ...
... First, if the equation is not complete, write out the correct formulas… 1. Use charges 2. Know the 7 Diatomic Elements: Make sure you know which elements are diatomic so you can write the correct equation. ...
Lecture 6
... are neutral and are assigned an oxidation state of zero. Similarly, when Na and K reacted with H2O they became positively charged. In this case the hydrogen in water, H+1 was reduced to its elemental state H20 ...
... are neutral and are assigned an oxidation state of zero. Similarly, when Na and K reacted with H2O they became positively charged. In this case the hydrogen in water, H+1 was reduced to its elemental state H20 ...
Chapter 3
... – how much reactant is consumed and how much product is formed – coefficients must be consistent with the Law of Conservation of Mass; atoms are neither created nor destroyed in a chemical reaction. – i.e. chemical equation must be balanced ...
... – how much reactant is consumed and how much product is formed – coefficients must be consistent with the Law of Conservation of Mass; atoms are neither created nor destroyed in a chemical reaction. – i.e. chemical equation must be balanced ...
Year 10 Chemistry Exam June 2011 Multiple Choice Section A
... 1. An aqueous solution is obtained when: a. a substance dissolves in any liquid b. a substance is dissolved in water c. when a substance is mixed with water and doesn’t dissolve d. water is removed from a substance 2. The graph shows the relative amount of chemical substances which can be taken up b ...
... 1. An aqueous solution is obtained when: a. a substance dissolves in any liquid b. a substance is dissolved in water c. when a substance is mixed with water and doesn’t dissolve d. water is removed from a substance 2. The graph shows the relative amount of chemical substances which can be taken up b ...
Document
... • Ca(OH)2 + H3PO4 H2O + Ca3(PO4)2 • Cr + S8 Cr2S3 • KClO3(s) Cl2(g) + O2(g) • Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen sulfide gas. • Fe2O3(s) + Al(s) Fe(s) + Al2O3(s) ...
... • Ca(OH)2 + H3PO4 H2O + Ca3(PO4)2 • Cr + S8 Cr2S3 • KClO3(s) Cl2(g) + O2(g) • Solid iron(III) sulfide reacts with gaseous hydrogen chloride to form solid iron(III) chloride and hydrogen sulfide gas. • Fe2O3(s) + Al(s) Fe(s) + Al2O3(s) ...
RXN-4-STUDENTS - Rothschild Science
... element you have NH3 (one nitrogen, three hydrogen)- DON’T mess with these!! Coefficients – small whole number that appears ...
... element you have NH3 (one nitrogen, three hydrogen)- DON’T mess with these!! Coefficients – small whole number that appears ...
Atomic Weights Average Atomic Masses
... • Relative atomic mass: average masses of isotopes: – Naturally occurring C: 98.892 % 12C + 1.108 % 13C. • Average mass of C: • (0.98892)(12 amu) + (0.01108)(13.00335) = 12.011 amu. • Atomic weight (AW) is also known as average atomic mass (atomic weight). • Atomic weights are listed on the periodic ...
... • Relative atomic mass: average masses of isotopes: – Naturally occurring C: 98.892 % 12C + 1.108 % 13C. • Average mass of C: • (0.98892)(12 amu) + (0.01108)(13.00335) = 12.011 amu. • Atomic weight (AW) is also known as average atomic mass (atomic weight). • Atomic weights are listed on the periodic ...
Problem
... Repeat the calculation of flame temperature if 10% excess of air is used. Repeat the calculation for a 10% deficiency of air. Assume that the combustion reaction is only 95% complete. Calculate the temperature for a stoichiometric mixture of propane and air. Careful and accurate measurements of the ...
... Repeat the calculation of flame temperature if 10% excess of air is used. Repeat the calculation for a 10% deficiency of air. Assume that the combustion reaction is only 95% complete. Calculate the temperature for a stoichiometric mixture of propane and air. Careful and accurate measurements of the ...
TERM 2 Unit 3 YR 9 SCI It is elementary
... understandings of atomic structure. Students model an atom according to currently accepted understandings. They will identify patterns in atomic structure that allow prediction of the products of chemical reactions and are reflected by the periodic table. They recognise that new substances are forme ...
... understandings of atomic structure. Students model an atom according to currently accepted understandings. They will identify patterns in atomic structure that allow prediction of the products of chemical reactions and are reflected by the periodic table. They recognise that new substances are forme ...
Stoichiometry
Stoichiometry /ˌstɔɪkiˈɒmɨtri/ is the calculation of relative quantities of reactants and products in chemical reactions.Stoichiometry is founded on the law of conservation of mass where the total mass of the reactants equals the total mass of the products leading to the insight that the relations among quantities of reactants and products typically form a ratio of positive integers. This means that if the amounts of the separate reactants are known, then the amount of the product can be calculated. Conversely, if one reactant has a known quantity and the quantity of product can be empirically determined, then the amount of the other reactants can also be calculated.As seen in the image to the right, where the balanced equation is:CH4 + 2 O2 → CO2 + 2 H2O.Here, one molecule of methane reacts with two molecules of oxygen gas to yield one molecule of carbon dioxide and two molecules of water. Stoichiometry measures these quantitative relationships, and is used to determine the amount of products/reactants that are produced/needed in a given reaction. Describing the quantitative relationships among substances as they participate in chemical reactions is known as reaction stoichiometry. In the example above, reaction stoichiometry measures the relationship between the methane and oxygen as they react to form carbon dioxide and water.Because of the well known relationship of moles to atomic weights, the ratios that are arrived at by stoichiometry can be used to determine quantities by weight in a reaction described by a balanced equation. This is called composition stoichiometry.Gas stoichiometry deals with reactions involving gases, where the gases are at a known temperature, pressure, and volume and can be assumed to be ideal gases. For gases, the volume ratio is ideally the same by the ideal gas law, but the mass ratio of a single reaction has to be calculated from the molecular masses of the reactants and products. In practice, due to the existence of isotopes, molar masses are used instead when calculating the mass ratio.