AP - 04 - Reactions in Aqueous Solutions
... H2S, S8, Na2SO3, and SO42(a) When bonded to a nonmetal, hydrogen has an oxidation number of +1 (rule 3b). Because the H2S molecule is neutral, the sum of the oxidation numbers must equal zero (rule 4). Letting x equal the oxidation number of S, we have 2(+1) + x = 0. Thus, S has an oxidation number ...
... H2S, S8, Na2SO3, and SO42(a) When bonded to a nonmetal, hydrogen has an oxidation number of +1 (rule 3b). Because the H2S molecule is neutral, the sum of the oxidation numbers must equal zero (rule 4). Letting x equal the oxidation number of S, we have 2(+1) + x = 0. Thus, S has an oxidation number ...
writing chemical equations
... 2. Solid calcium reacts with oxygen gas. 3. Solutions of aluminum chloride & sodium carbonate are mixed. 4. Liquid magnesium bromide is decomposed at high temperature. 5. Solid nickel is reacted with aqueous magnesium sulfate. 6. Chlorine gas is reacted with aqueous potassium bromide. 7. Solid magne ...
... 2. Solid calcium reacts with oxygen gas. 3. Solutions of aluminum chloride & sodium carbonate are mixed. 4. Liquid magnesium bromide is decomposed at high temperature. 5. Solid nickel is reacted with aqueous magnesium sulfate. 6. Chlorine gas is reacted with aqueous potassium bromide. 7. Solid magne ...
remaster unit 8A + 7
... • What is the molarity of a solution with 2.0 moles of CaCl2 in 4 L of H2O? • What is the molality of a solution with 4.0 moles of CaCl2 in 6 L of H2O? • What is the boiling point of a solution with 4 m CaCl2 in water? ...
... • What is the molarity of a solution with 2.0 moles of CaCl2 in 4 L of H2O? • What is the molality of a solution with 4.0 moles of CaCl2 in 6 L of H2O? • What is the boiling point of a solution with 4 m CaCl2 in water? ...
Thermochemistry and Measuring Energy Change Complete NOTES
... Standard Enthalpy of Combustion The experimental determination of Hfo values is often difficult or impossible. Combustion of organic compounds involves the reaction with molecular oxygen to form gaseous carbon dioxide and liquid water, as seen in this example with sucrose: ...
... Standard Enthalpy of Combustion The experimental determination of Hfo values is often difficult or impossible. Combustion of organic compounds involves the reaction with molecular oxygen to form gaseous carbon dioxide and liquid water, as seen in this example with sucrose: ...
ionization energies
... • Why is there such wide variation in the reactivity and physical properties of elements? • Why is there periodic repetition (periodicity) of the chemical/physical properties of elements as we move across the periodic table? ...
... • Why is there such wide variation in the reactivity and physical properties of elements? • Why is there periodic repetition (periodicity) of the chemical/physical properties of elements as we move across the periodic table? ...
Mass Relationships in Chemical Reactions
... It is process in which one or more pure substances are converted into one or more different pure substance. All chemical reactions involve a change in substances and a change in energy. Neither matter nor energy is created or destroyed in a chemical reaction, only changed. ...
... It is process in which one or more pure substances are converted into one or more different pure substance. All chemical reactions involve a change in substances and a change in energy. Neither matter nor energy is created or destroyed in a chemical reaction, only changed. ...
AP Chemistry Standards and Benchmarks
... These descriptive facts, including chemistry involved in environmental and societal issues, should not be isolated form the principles being studied but should be taught throughout the course to illustrate and illuminate the principles. The following areas should be covered: • chemical reactivity an ...
... These descriptive facts, including chemistry involved in environmental and societal issues, should not be isolated form the principles being studied but should be taught throughout the course to illustrate and illuminate the principles. The following areas should be covered: • chemical reactivity an ...
L2S08b
... Hess’s Law Hess’s law states that if a reaction is carried out in a series of steps, ∆H for the reaction will be equal to the sum of the enthalpy changes for the individual steps. Hess pointed out that the heat absorbed (or evolved) in a given chemical reaction is the same whether the process takes ...
... Hess’s Law Hess’s law states that if a reaction is carried out in a series of steps, ∆H for the reaction will be equal to the sum of the enthalpy changes for the individual steps. Hess pointed out that the heat absorbed (or evolved) in a given chemical reaction is the same whether the process takes ...
video slide
... Chemical reactions make and break chemical bonds Chemical reactions lead to new arrangements of atoms The starting molecules of a chemical reaction are called reactants The final molecules of a chemical reaction are called products ...
... Chemical reactions make and break chemical bonds Chemical reactions lead to new arrangements of atoms The starting molecules of a chemical reaction are called reactants The final molecules of a chemical reaction are called products ...
Example 1: An experiment shows that 64g of
... d. Work out the number of mol H2O and the number of mol CuSO4 originally present in the crystals. e. Work out the number of mol H2O which combine with 1 mol CuSO4 in the crystals. f. ...
... d. Work out the number of mol H2O and the number of mol CuSO4 originally present in the crystals. e. Work out the number of mol H2O which combine with 1 mol CuSO4 in the crystals. f. ...
Example 1: An experiment shows that 64g of
... d. Work out the number of mol H2O and the number of mol CuSO4 originally present in the crystals. e. Work out the number of mol H2O which combine with 1 mol CuSO4 in the crystals. f. ...
... d. Work out the number of mol H2O and the number of mol CuSO4 originally present in the crystals. e. Work out the number of mol H2O which combine with 1 mol CuSO4 in the crystals. f. ...
Theoretical Study of Atomic Layer Deposition Reaction Mechanism
... 3.1.4. P5 + H2O. Similar to the P3 + H2O reaction, the second water molecule is attached to the aluminum atom of P5 by a barrierless association process. The heat released is 22.0 kcal/mol for the formation of the intermediate complex P6, slightly more than the heat released in P3 + H2O f P4. The tr ...
... 3.1.4. P5 + H2O. Similar to the P3 + H2O reaction, the second water molecule is attached to the aluminum atom of P5 by a barrierless association process. The heat released is 22.0 kcal/mol for the formation of the intermediate complex P6, slightly more than the heat released in P3 + H2O f P4. The tr ...
Fall Semester Review Packet
... 10. Explain the difference between a molecule (covalent compound) and an ionic compound. Include the interaction between valence electrons and the types of bonds for each. 11. There are many components of a scientific experiment, including a manipulated variable, a responding variable and a control. ...
... 10. Explain the difference between a molecule (covalent compound) and an ionic compound. Include the interaction between valence electrons and the types of bonds for each. 11. There are many components of a scientific experiment, including a manipulated variable, a responding variable and a control. ...
Test 8 Review
... cause reactions. An effective collision is one in which the colliding particles approach each other at the proper angle and with the proper amount of energy to cause a reaction. The greater the rate of effective collisions is, the greater the reaction rate is. Reaction mechanisms. Effective collisio ...
... cause reactions. An effective collision is one in which the colliding particles approach each other at the proper angle and with the proper amount of energy to cause a reaction. The greater the rate of effective collisions is, the greater the reaction rate is. Reaction mechanisms. Effective collisio ...
Loeblein chemistry clicker questions2013
... 9. If you had a water bottle with very soft sides. When you open your suitcase in Boston, the bottle would look A. squished B. same size C. puffed out ...
... 9. If you had a water bottle with very soft sides. When you open your suitcase in Boston, the bottle would look A. squished B. same size C. puffed out ...
Example 1: An experiment shows that 64g of
... d. Work out the number of mol H2O and the number of mol CuSO4 originally present in the crystals. e. Work out the number of mol H2O which combine with 1 mol CuSO4 in the crystals. f. ...
... d. Work out the number of mol H2O and the number of mol CuSO4 originally present in the crystals. e. Work out the number of mol H2O which combine with 1 mol CuSO4 in the crystals. f. ...
R E V I E W -- P R A C T I C E E X A
... 82. Which of the following statements is FALSE: a. Ionization energies decrease as you move down a group b. Atomic radius generally increases as you move from right to left within a period c. Shielding effect is constant as you move from left to right across a period d. Electron affinities decrease ...
... 82. Which of the following statements is FALSE: a. Ionization energies decrease as you move down a group b. Atomic radius generally increases as you move from right to left within a period c. Shielding effect is constant as you move from left to right across a period d. Electron affinities decrease ...
Key Words Questions and Problems
... many grams of NO2 will be produced? Which comProblems pound is the limiting reagent? Calculate the number of moles of the excess reagent remaining at the end •• 3.81 Consider the reaction of the reaction. 2A B ¡ C •• 3.85 Propane (C3H8) is a component of natural gas and is (a) In the diagram here ...
... many grams of NO2 will be produced? Which comProblems pound is the limiting reagent? Calculate the number of moles of the excess reagent remaining at the end •• 3.81 Consider the reaction of the reaction. 2A B ¡ C •• 3.85 Propane (C3H8) is a component of natural gas and is (a) In the diagram here ...
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.