File
... ______1. Which of the following will increase the Ksp of PbCl2 ? A) Addition of HCl to the solution B) Addition of Pb(NO3)2 to the solution C) An increase in temperature D) All of these. ______2. AgCl would be LEAST soluble in a solution of 1.00 molar A) HNO3 B) AgNO3 C) HCl D) BaCl2 ______3. Methan ...
... ______1. Which of the following will increase the Ksp of PbCl2 ? A) Addition of HCl to the solution B) Addition of Pb(NO3)2 to the solution C) An increase in temperature D) All of these. ______2. AgCl would be LEAST soluble in a solution of 1.00 molar A) HNO3 B) AgNO3 C) HCl D) BaCl2 ______3. Methan ...
Chapter 3 Stoichiometry: Calculations with Chemical
... How many grams of lead (II) carbonate should decompose completely to produce 20.0 g of lead (II) oxide? (a). 0.41 g (b). 20.0 g (c) 23.9 g (d). 20.9 g Explanation: Ensure that the equation is balanced. Convert the grams of lead (II) oxide to moles of lead (II) oxide. Using the stoichiometric factor ...
... How many grams of lead (II) carbonate should decompose completely to produce 20.0 g of lead (II) oxide? (a). 0.41 g (b). 20.0 g (c) 23.9 g (d). 20.9 g Explanation: Ensure that the equation is balanced. Convert the grams of lead (II) oxide to moles of lead (II) oxide. Using the stoichiometric factor ...
4th NOTES - Idaho State University
... For the case where the heat capacity of a calorimeter and its contents are known. Qtot = C C = heat capacity of the calorimeter and substances in it! C = Ccalorimeter + Ccontents If the Reaction is carried out in Dilute aqeous solution and Ccal = 0 Q = sp.htH2O * mH2O * T sp. ht. = J/(g ...
... For the case where the heat capacity of a calorimeter and its contents are known. Qtot = C C = heat capacity of the calorimeter and substances in it! C = Ccalorimeter + Ccontents If the Reaction is carried out in Dilute aqeous solution and Ccal = 0 Q = sp.htH2O * mH2O * T sp. ht. = J/(g ...
Section II - School District 27J
... solution. Determine the molar mass of the acid if the sample required 45.00 mL of 0.1000 M sodium hydroxide to reach its endpoint. c. What is the molecular formula for this acid? (EC ~ NAME IT!) ...
... solution. Determine the molar mass of the acid if the sample required 45.00 mL of 0.1000 M sodium hydroxide to reach its endpoint. c. What is the molecular formula for this acid? (EC ~ NAME IT!) ...
The Mole - C405 Chemistry
... C.8.E Perform stoichiometric calculations, including determination of mass relationships between reactants and products, calculation of limiting reagents, and percent yield ...
... C.8.E Perform stoichiometric calculations, including determination of mass relationships between reactants and products, calculation of limiting reagents, and percent yield ...
AP Chem Mr. Dehne Name: ___________ Date: Per#: ___ AP
... manganese chloride compound (MnClx). What is the formula of the manganese chloride compound produced in the reaction? 3. A 15.0L tank is filled with H2 to a pressure 2.00x102atm. How many balloons (each 2.00L) can be inflated to a pressure of 1.00atm from the tank? Assume that there is no temperatur ...
... manganese chloride compound (MnClx). What is the formula of the manganese chloride compound produced in the reaction? 3. A 15.0L tank is filled with H2 to a pressure 2.00x102atm. How many balloons (each 2.00L) can be inflated to a pressure of 1.00atm from the tank? Assume that there is no temperatur ...
Chapter 3 Lecture notes
... Specialized cells in the stomach release HCl to aid digestion. If they release too much, the excess can be neutralized with antacids. A common antacid contains magnesium hydroxide, which reacts with the acid to form water and magnesium chloride solution. As a government chemist testing commercial an ...
... Specialized cells in the stomach release HCl to aid digestion. If they release too much, the excess can be neutralized with antacids. A common antacid contains magnesium hydroxide, which reacts with the acid to form water and magnesium chloride solution. As a government chemist testing commercial an ...
Name LeChatallier`s Principle © Van Der Sluys, 2004 Some
... reactions will become the same and the reaction is said to have reached equilibrium. However it is possible to disturb this equilibrium by changing the conditions. LeChatallier’s Priniciple is often used to describe the effect of changing the conditions of an equilibrium system. Simply stated, when ...
... reactions will become the same and the reaction is said to have reached equilibrium. However it is possible to disturb this equilibrium by changing the conditions. LeChatallier’s Priniciple is often used to describe the effect of changing the conditions of an equilibrium system. Simply stated, when ...
Brønsted acid
... 4. The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds. In these cases, its oxidation number is –1. 5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1. 6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to ...
... 4. The oxidation number of hydrogen is +1 except when it is bonded to metals in binary compounds. In these cases, its oxidation number is –1. 5. Group IA metals are +1, IIA metals are +2 and fluorine is always –1. 6. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to ...
The Mole - semphchem
... A compound has an empirical formula of NO2. The colourless liquid, used in rocket engines has a molar mass of 92.0 g/mole. What is the molecular formula of this substance? ...
... A compound has an empirical formula of NO2. The colourless liquid, used in rocket engines has a molar mass of 92.0 g/mole. What is the molecular formula of this substance? ...
Reactions in Aqueous Solution (Brown 13th-Fossum
... • Arrhenius: substances that increase the concentration of H+ when dissolved in water. • Brønsted and Lowry: proton donors. Bases – Taste bitter and have a high pH. (Turn litmus paper blue.) • Arrhenius: Increase the concentration of OH− when dissolved in water. • Brønsted and Lowry: proton acceptor ...
... • Arrhenius: substances that increase the concentration of H+ when dissolved in water. • Brønsted and Lowry: proton donors. Bases – Taste bitter and have a high pH. (Turn litmus paper blue.) • Arrhenius: Increase the concentration of OH− when dissolved in water. • Brønsted and Lowry: proton acceptor ...
Moles
... Empirical Formula = the formula of a compound expressed as the smallest possible whole-number ratio of subscripts of the elements in the formula Molecular Formula = the formula of a compound in which the subscripts give the actual number of each element in the formula ...
... Empirical Formula = the formula of a compound expressed as the smallest possible whole-number ratio of subscripts of the elements in the formula Molecular Formula = the formula of a compound in which the subscripts give the actual number of each element in the formula ...
practice-exam-2
... 4. [7 points] What is the correct name for H3PO3? (a) phosphate (b) phosphorous acid (c) hydrogen phosphite (d) phosphoric acid (e) perphosphoric acid 5. [7 points] What is the empirical formula of barium perchlorate? (a) BaClO3 (b) Ba(ClO3)2 (c) BaClO4 (d) Ba2ClO4 ...
... 4. [7 points] What is the correct name for H3PO3? (a) phosphate (b) phosphorous acid (c) hydrogen phosphite (d) phosphoric acid (e) perphosphoric acid 5. [7 points] What is the empirical formula of barium perchlorate? (a) BaClO3 (b) Ba(ClO3)2 (c) BaClO4 (d) Ba2ClO4 ...
File
... atomic emission spectra; Bohr model of the hydrogen atom including explanation of H line spectrum and orbits, electron cloud and the probability model, wave/particle duality of electrons revisited, relate electron configurations of atoms to the Bohr and electron cloud models, describe the concepts o ...
... atomic emission spectra; Bohr model of the hydrogen atom including explanation of H line spectrum and orbits, electron cloud and the probability model, wave/particle duality of electrons revisited, relate electron configurations of atoms to the Bohr and electron cloud models, describe the concepts o ...
Objective 4
... One mole equals 6.02 x 1023 (also known as Avogadro's number). One mole of hydrogen atoms (6.02 x 1023 H atoms) weighs 1 g. (And so forth….) ...
... One mole equals 6.02 x 1023 (also known as Avogadro's number). One mole of hydrogen atoms (6.02 x 1023 H atoms) weighs 1 g. (And so forth….) ...
Molar Mass and Formulas
... Benzopyrene, C20H12 • Benzopyrene is found in nature from the eruption of volcanoes and forest fires. It is also produced by burning plants, wood, coal, and operating cars, trucks and other ...
... Benzopyrene, C20H12 • Benzopyrene is found in nature from the eruption of volcanoes and forest fires. It is also produced by burning plants, wood, coal, and operating cars, trucks and other ...
Atoms and Elements: Are they Related?
... A burning match is a good example of a chemical reaction. Application of a spark to the chemicals on the match head start the chemical reaction. Signs of a chemical change – heat given off, ...
... A burning match is a good example of a chemical reaction. Application of a spark to the chemicals on the match head start the chemical reaction. Signs of a chemical change – heat given off, ...
The Mole & Stoicheometry
... C.8.E Perform stoichiometric calculations, including determination of mass relationships between reactants and products, calculation of limiting reagents, and percent yield ...
... C.8.E Perform stoichiometric calculations, including determination of mass relationships between reactants and products, calculation of limiting reagents, and percent yield ...
Chapter 8
... Use Avogadro’s Number to determine the number of atoms in 1 mole 1 mole Al = 6.02 x 1023 atoms Use this as a conversion factor for atoms-to-moles 1 mol Al 2.23x 10 Al atoms x 0.370mol Al ...
... Use Avogadro’s Number to determine the number of atoms in 1 mole 1 mole Al = 6.02 x 1023 atoms Use this as a conversion factor for atoms-to-moles 1 mol Al 2.23x 10 Al atoms x 0.370mol Al ...
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.