Chemistry Cram Sheet
... The average atomic mass is an average of all the isotopes of an element. (This is why the atomic mass on the periodic table is a decimal. That should make sense – you can’t have .01 neutrons!) Average Atomic Mass = (% abundance x mass number)1 + (% abundance + mass number)2 + … There are two isotope ...
... The average atomic mass is an average of all the isotopes of an element. (This is why the atomic mass on the periodic table is a decimal. That should make sense – you can’t have .01 neutrons!) Average Atomic Mass = (% abundance x mass number)1 + (% abundance + mass number)2 + … There are two isotope ...
Cosmetology Learning Module 12
... substances The result of a chemical reaction that creates new chemicals that have new chemical and physical properties Oxidation of haircolor Polymerization of acrylic (methacrylate) nail ...
... substances The result of a chemical reaction that creates new chemicals that have new chemical and physical properties Oxidation of haircolor Polymerization of acrylic (methacrylate) nail ...
Quantitative Chemistry
... 2. Work out relative formula mass (RFM) for each compound in the equation 3. Below the RFM write out the mass given in the qs 4. Work out the scale factor by dividing/multiplying mass given by RFM of that compound 5. Do the same thing to the value you are trying to calculate a mass for – using the s ...
... 2. Work out relative formula mass (RFM) for each compound in the equation 3. Below the RFM write out the mass given in the qs 4. Work out the scale factor by dividing/multiplying mass given by RFM of that compound 5. Do the same thing to the value you are trying to calculate a mass for – using the s ...
Physical and Chemical Changes
... It’s a chemical change if.... A precipitate is formed. A precipitate is a solid that forms and separates out from a liquid mixture. This goes along with the “a new substance is formed” ...
... It’s a chemical change if.... A precipitate is formed. A precipitate is a solid that forms and separates out from a liquid mixture. This goes along with the “a new substance is formed” ...
SPRING 2002 Test 2 1. Which of the following statements is
... 6. Consider the equilibrium reaction, N2(g) + O2(g) <=> 2NO(g), where Kc = [NO]2/[N2][O2]. The equilibrium constant for the reaction, 2N2(g) + 2O2(g) <=> 4NO(g) is: A. (1/Kc)4 B. (Kc)4 C. (Kc)1/2 D. (1/Kc)2 E. (Kc)2 Ans. E 7. Which of the following statements is FALSE: A. At equilibrium, the concent ...
... 6. Consider the equilibrium reaction, N2(g) + O2(g) <=> 2NO(g), where Kc = [NO]2/[N2][O2]. The equilibrium constant for the reaction, 2N2(g) + 2O2(g) <=> 4NO(g) is: A. (1/Kc)4 B. (Kc)4 C. (Kc)1/2 D. (1/Kc)2 E. (Kc)2 Ans. E 7. Which of the following statements is FALSE: A. At equilibrium, the concent ...
Chapter 1
... b) The atomic weight of boron is reported as 10.81, yet no atom of boron has the mass of 10.81 amu. Explain. Atomic weights are really average atomic masses, the sum of the mass of each naturally occurring isotope of an element times its fractional abundance. Each B atom will have the mass of one of ...
... b) The atomic weight of boron is reported as 10.81, yet no atom of boron has the mass of 10.81 amu. Explain. Atomic weights are really average atomic masses, the sum of the mass of each naturally occurring isotope of an element times its fractional abundance. Each B atom will have the mass of one of ...
Chapter 7
... 1. the mass in grams of one mole of a pure substance (element or compound) 2. use the periodic table to find the mass 3. What is the molar mass of helium? 4.0 g He mole 4. will be used as a conversion factor ...
... 1. the mass in grams of one mole of a pure substance (element or compound) 2. use the periodic table to find the mass 3. What is the molar mass of helium? 4.0 g He mole 4. will be used as a conversion factor ...
Chemistry Review 3
... oxides that glow brightly when heated to a high temperature. During a test, a propane lantern is operated for three hours and consumes 5.0 moles of propane from the lantern's tank. The balanced equation below represents the combustion of propane. C3H8 + 5O2 → 3CO2 + 4H2O + energy Determine the total ...
... oxides that glow brightly when heated to a high temperature. During a test, a propane lantern is operated for three hours and consumes 5.0 moles of propane from the lantern's tank. The balanced equation below represents the combustion of propane. C3H8 + 5O2 → 3CO2 + 4H2O + energy Determine the total ...
Chapter 7 Lecture
... Molecular, Complete Ionic, and Net Ionic Equations A molecular equation is a chemical equation showing the complete, neutral formulas for every compound in a reaction. A complete ionic equation is a chemical equation showing all of the species as they are actually present in solution. A net ionic e ...
... Molecular, Complete Ionic, and Net Ionic Equations A molecular equation is a chemical equation showing the complete, neutral formulas for every compound in a reaction. A complete ionic equation is a chemical equation showing all of the species as they are actually present in solution. A net ionic e ...
File
... in plastic foams (used as foam insulation, foam trays, and cartons). CFC-12, which is pure CF2Cl2, was made by reacting carbon tetrachloride with gaseous hydrogen fluoride. The carbon tetrachloride was produced by reacting methane with chlorine. Draw structural formula equations to represent these t ...
... in plastic foams (used as foam insulation, foam trays, and cartons). CFC-12, which is pure CF2Cl2, was made by reacting carbon tetrachloride with gaseous hydrogen fluoride. The carbon tetrachloride was produced by reacting methane with chlorine. Draw structural formula equations to represent these t ...
The Mole - Rothschild Science
... One formula unit of calcium carbonate reacts to form one formula unit of calcium oxide and one molecule of carbon dioxide. One mole of calcium carbonate reacts to form one mole of calcium oxide and one mole of carbon dioxide. ...
... One formula unit of calcium carbonate reacts to form one formula unit of calcium oxide and one molecule of carbon dioxide. One mole of calcium carbonate reacts to form one mole of calcium oxide and one mole of carbon dioxide. ...
Measuring and Calculating
... 3-dimensional arrangement of atoms in a molecule electron pairs are drawn as either dots or straight lines bonded pairs are between atoms while nonbonded pairs are only on one atom To draw a structure, o calculate the total number of valence electron pairs in your molecule. Next bond all ato ...
... 3-dimensional arrangement of atoms in a molecule electron pairs are drawn as either dots or straight lines bonded pairs are between atoms while nonbonded pairs are only on one atom To draw a structure, o calculate the total number of valence electron pairs in your molecule. Next bond all ato ...
Practice Unit D Exam - mvhs
... Then the student pours 25 mL of the 6 M HNO3 into a beaker and adds a 0.6489 g sample of the alloy. After the sample completely reacts with the acid, some saturated NaCl(aq) is added to the beaker, resulting in the formation of an AgCl precipitate. Additional NaCl(aq) is added until no more precipit ...
... Then the student pours 25 mL of the 6 M HNO3 into a beaker and adds a 0.6489 g sample of the alloy. After the sample completely reacts with the acid, some saturated NaCl(aq) is added to the beaker, resulting in the formation of an AgCl precipitate. Additional NaCl(aq) is added until no more precipit ...
Chapter 4 Reactions in Aqueous Solutions
... Ni2+(aq) + 2e Ni(s) – Multiply by a common factor to equalize electrons (the number of electrons lost must equal number of electrons gained) 2 [Al(s) Al3+(aq) + 3e ] 3 [Ni2+(aq) + 2e Ni(s) ] ...
... Ni2+(aq) + 2e Ni(s) – Multiply by a common factor to equalize electrons (the number of electrons lost must equal number of electrons gained) 2 [Al(s) Al3+(aq) + 3e ] 3 [Ni2+(aq) + 2e Ni(s) ] ...
File
... cannot make the Law of Conseravation of mass disappear, they are good, but NOT that good. Reaction Rates: STSE: Smog, Catalytic Converters: All cars today must have catalytic converters to minimize pollutants or smog. The word "smog" means "smoke and fog". Engine exhaust contains NO, NO2, unburned h ...
... cannot make the Law of Conseravation of mass disappear, they are good, but NOT that good. Reaction Rates: STSE: Smog, Catalytic Converters: All cars today must have catalytic converters to minimize pollutants or smog. The word "smog" means "smoke and fog". Engine exhaust contains NO, NO2, unburned h ...
NYS Regents Chemistry June 21, 2002
... 1: II. PERIODIC TABLE\1. Properties of Elements\A. Metals\1. Metals - (32) 2: II. PERIODIC TABLE\2. Valence Electrons\A. Electron / Ionic Configuration\2. Ionic Configuration - (10, 30) 2: II. PERIODIC TABLE\4. Properties of Periods\C. Electronegativity\1. Electronegativity - (11, 13) 1: II. PERIODI ...
... 1: II. PERIODIC TABLE\1. Properties of Elements\A. Metals\1. Metals - (32) 2: II. PERIODIC TABLE\2. Valence Electrons\A. Electron / Ionic Configuration\2. Ionic Configuration - (10, 30) 2: II. PERIODIC TABLE\4. Properties of Periods\C. Electronegativity\1. Electronegativity - (11, 13) 1: II. PERIODI ...
Tutorial 1
... 9. All alkali metals react with water to produce hydrogen gas and the corresponding alkali metal hydroxide. A typical reaction is that between lithium and water. Li (s) + H2O (l) LiOH (aq) + H2 (g) (not balanced) a. How many moles of H2 will be formed by the complete reaction of 6.23 moles of Li w ...
... 9. All alkali metals react with water to produce hydrogen gas and the corresponding alkali metal hydroxide. A typical reaction is that between lithium and water. Li (s) + H2O (l) LiOH (aq) + H2 (g) (not balanced) a. How many moles of H2 will be formed by the complete reaction of 6.23 moles of Li w ...
CHEMSTRY FREE-RESPONSE QUESTIONS (Form B)
... g = the mass, in grams, of the sample of the iron(II) compound M= the molarity of the MnO4-(aq)) used as the titrant V = the volume, in liters, of MnO4-(aq)) added to reach the end point In terms of these variables, the number of moles of MnO4-(aq)) added to reach the end point of the titration is e ...
... g = the mass, in grams, of the sample of the iron(II) compound M= the molarity of the MnO4-(aq)) used as the titrant V = the volume, in liters, of MnO4-(aq)) added to reach the end point In terms of these variables, the number of moles of MnO4-(aq)) added to reach the end point of the titration is e ...
Mole Introduction
... determine the mass of elements by comparing their “RELATIVE MASS”, which is a mass ratio between two elements. Example 1: Reaction: H2 + Cl2 2HCl The reaction between 2.74g of hydrogen gas and 97.26g of chlorine gas makes 100g of hydrogen chloride. What is the relative mass of a chlorine atom to a ...
... determine the mass of elements by comparing their “RELATIVE MASS”, which is a mass ratio between two elements. Example 1: Reaction: H2 + Cl2 2HCl The reaction between 2.74g of hydrogen gas and 97.26g of chlorine gas makes 100g of hydrogen chloride. What is the relative mass of a chlorine atom to a ...
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.