Ch. 7 & 8 Notes (Chemical Reactions) teacher
... right yields products are on the __________ side. The arrow means “________”, or “reacts to produce” when read aloud. ...
... right yields products are on the __________ side. The arrow means “________”, or “reacts to produce” when read aloud. ...
DALTON`S ATOMIC THEORY - 1808: Publication of Dalton`s "A New
... Matter is composed of small, chemically indivisible ATOMS ELEMENTS are kinds of matter that contain only a single kind of atom. All the atoms of an element have identical chemical properties. COMPOUNDS are kinds of matter that are composed of atoms of two or more ELEMENTS which are combined in simpl ...
... Matter is composed of small, chemically indivisible ATOMS ELEMENTS are kinds of matter that contain only a single kind of atom. All the atoms of an element have identical chemical properties. COMPOUNDS are kinds of matter that are composed of atoms of two or more ELEMENTS which are combined in simpl ...
Chapter 13 Notes
... Next count the number of atoms of each element on both sides of the yields arrow. If the number of atoms of each element on the left side of the arrow equals the number on the right, the equation is balanced and no further changes are needed. If they are not the same, then we balance the equation by ...
... Next count the number of atoms of each element on both sides of the yields arrow. If the number of atoms of each element on the left side of the arrow equals the number on the right, the equation is balanced and no further changes are needed. If they are not the same, then we balance the equation by ...
Writing Chemical Equations KClO3 O2 (g) + KCl (s) Balancing
... one atom of oxygen and ended with 2 atoms of oxygen. We cannot change the numbers at the bottom of the symbols because that is how the formulas must be written. To balance the equation we put numbers in front of the formulas to multiply the number of atoms in each formula. 2H2O 2H2 + O2 This gives ...
... one atom of oxygen and ended with 2 atoms of oxygen. We cannot change the numbers at the bottom of the symbols because that is how the formulas must be written. To balance the equation we put numbers in front of the formulas to multiply the number of atoms in each formula. 2H2O 2H2 + O2 This gives ...
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Second review [Compatibility Mode]
... When 0.0300 mol of Na was added to 100.0 g of water, the temperature of the resulting solution rose from 25.0 oC to 37.9 oC. If the specific heat of the solution was 4.18 J g-1 K-1, calculate ? H, in kJ, for the reaction as written. ...
... When 0.0300 mol of Na was added to 100.0 g of water, the temperature of the resulting solution rose from 25.0 oC to 37.9 oC. If the specific heat of the solution was 4.18 J g-1 K-1, calculate ? H, in kJ, for the reaction as written. ...
IntroRedoxDCIAns
... b. Identify two characteristics common to these equations. The first three reactions show an element, in this case oxygen, converted to the combined form of oxygen in a compound. An element was converted to a compound in the reactions. In the fourth reaction, a compound decomposed into its elements. ...
... b. Identify two characteristics common to these equations. The first three reactions show an element, in this case oxygen, converted to the combined form of oxygen in a compound. An element was converted to a compound in the reactions. In the fourth reaction, a compound decomposed into its elements. ...
CHEMICAL REACTIONS
... reactants (the molecules shown on the left of the arrow) into products (the molecules shown on the right of the arrow). • A + sign separates molecules on the same side • The arrow is read as “yields” • Example C + O2 CO2 • This reads “carbon plus oxygen react to yield carbon dioxide” ...
... reactants (the molecules shown on the left of the arrow) into products (the molecules shown on the right of the arrow). • A + sign separates molecules on the same side • The arrow is read as “yields” • Example C + O2 CO2 • This reads “carbon plus oxygen react to yield carbon dioxide” ...
Chapter 6: Chemistry in Biology
... An __________ is a pure substance that cannot be broken down into other substances by physical or chemical means. ...
... An __________ is a pure substance that cannot be broken down into other substances by physical or chemical means. ...
final exam review packet
... 42. The concentration of a solution can be calculated by solving for M, which stands for __________________ . A. You have 39.2 L of solution that contains 49.21 mol of sodium chloride, NaCl. What is the molarity of that solution? ...
... 42. The concentration of a solution can be calculated by solving for M, which stands for __________________ . A. You have 39.2 L of solution that contains 49.21 mol of sodium chloride, NaCl. What is the molarity of that solution? ...
Unit 3C Standards for Quiz
... 3. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to calculate the mass of products and reactants. As a basis for understanding this concept, students know: a. how to describe chemical reactions by writing balanced equations. b. the q ...
... 3. The conservation of atoms in chemical reactions leads to the principle of conservation of matter and the ability to calculate the mass of products and reactants. As a basis for understanding this concept, students know: a. how to describe chemical reactions by writing balanced equations. b. the q ...
Step by Step Stoichiometry
... These problems will ask you to calculate the amount of one substance, in grams, that will be needed to react or be produced from a given mass for another substance. The plan for solving these kinds of problems: Mass of given amount of given in moles amount of unknown in moles mass of ...
... These problems will ask you to calculate the amount of one substance, in grams, that will be needed to react or be produced from a given mass for another substance. The plan for solving these kinds of problems: Mass of given amount of given in moles amount of unknown in moles mass of ...
General Chemistry - Review for final exam: (Make sure you bring
... d. KClO3 (Decomposition) e. CH4 + O2 (Combustion) 71. In the above reaction, NaCl + F2 NaF + Cl2, F is more or less reactive than Cl? 72. In the activity series of metals are the more reactive metals found on the top or the bottom of the chart? 73. What conditions in the reactants must be pres ...
... d. KClO3 (Decomposition) e. CH4 + O2 (Combustion) 71. In the above reaction, NaCl + F2 NaF + Cl2, F is more or less reactive than Cl? 72. In the activity series of metals are the more reactive metals found on the top or the bottom of the chart? 73. What conditions in the reactants must be pres ...
Practice questions
... The average atomic mass of Eu is 151.96 amu. There are only two naturally occurring isotopes of europium, 151Eu with a mass of 151.0 amu and 153Eu with a mass of 153.0 amu. The natural abundance of the 131Eu isotope must be approximately a) ...
... The average atomic mass of Eu is 151.96 amu. There are only two naturally occurring isotopes of europium, 151Eu with a mass of 151.0 amu and 153Eu with a mass of 153.0 amu. The natural abundance of the 131Eu isotope must be approximately a) ...
Introduction_to_Geochemistry_Pre-Lecture_Quiz
... Introduction to Geochemistry – Pre-lecture Quiz (1) True or False? (a) The diameter of an atom is less than the diameter of its nucleus. (b) The relative atomic mass of an atom is the mass of an atom relative to an atom of 12C. (c) p-orbitals can contain a maximum of 10 electrons. (d) The first ioni ...
... Introduction to Geochemistry – Pre-lecture Quiz (1) True or False? (a) The diameter of an atom is less than the diameter of its nucleus. (b) The relative atomic mass of an atom is the mass of an atom relative to an atom of 12C. (c) p-orbitals can contain a maximum of 10 electrons. (d) The first ioni ...
File - Mr. J`s Chemistry 4U
... T / F : A thermite reaction can produce temperatures in excess of 350o. ...
... T / F : A thermite reaction can produce temperatures in excess of 350o. ...
chapter 1 - Revsworld
... water. Determine the empirical formula of this compound. SHOW ALL WORK (a) (b) (c) (d) (e) ...
... water. Determine the empirical formula of this compound. SHOW ALL WORK (a) (b) (c) (d) (e) ...
Chemistry B11 Chapter 4 Chemical reactions
... Formula weight of H2O = 18 amu → molar mass = 18 g (mass of 1 mole H2O) Formula weight of NaCl = 58.5 amu → molar mass = 58.5 g (mass of 1 mole NaCl) Balance a chemical equation: in a balanced equation, there must be the same number of atoms of each element on both sides (the law of conservation of ...
... Formula weight of H2O = 18 amu → molar mass = 18 g (mass of 1 mole H2O) Formula weight of NaCl = 58.5 amu → molar mass = 58.5 g (mass of 1 mole NaCl) Balance a chemical equation: in a balanced equation, there must be the same number of atoms of each element on both sides (the law of conservation of ...
Chemical Reactions
... In a synthesis reaction two or more substances combine to form a more complex substance. A decomposition reaction is the opposite of synthesis and breaks down a compound into two or more substances. In a single replacement reaction, one substance in a compound is replaced by another, more active, su ...
... In a synthesis reaction two or more substances combine to form a more complex substance. A decomposition reaction is the opposite of synthesis and breaks down a compound into two or more substances. In a single replacement reaction, one substance in a compound is replaced by another, more active, su ...
Exam 1 Review
... Calculate ΔH using: Hess’s Law, heats of formation, bond dissociation energies Given ΔH for a reaction, how much heat is released when 20 g of product is formed? (hint – use the balanced chemical equation to solve) Find heat needed to change water at 20 °C to steam at 100 °C. Does entropy increase o ...
... Calculate ΔH using: Hess’s Law, heats of formation, bond dissociation energies Given ΔH for a reaction, how much heat is released when 20 g of product is formed? (hint – use the balanced chemical equation to solve) Find heat needed to change water at 20 °C to steam at 100 °C. Does entropy increase o ...
Stoichiometry
... Atomic mass is the mass of an atom in atomic mass units (amu) By definition: 1 atom 12C “weighs” 12 amu On this scale ...
... Atomic mass is the mass of an atom in atomic mass units (amu) By definition: 1 atom 12C “weighs” 12 amu On this scale ...
3a-General Reactions 2010
... a solution of silver nitrate to produce aqueous sodium nitrate and a precipitate of silver phosphate. Balanced equation: ? ...
... a solution of silver nitrate to produce aqueous sodium nitrate and a precipitate of silver phosphate. Balanced equation: ? ...
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.