Stoichiometry: Calculations with Chemical Formulas and Equations
... of 1 mol of a substance (i.e., g/mol). – The molar mass of an element is the mass number for the element that we find on the periodic table. – The formula weight (in amu’s) will be the same number as the molar mass (in g/mol). Stoichiometry © 2012 Pearson Education, Inc. ...
... of 1 mol of a substance (i.e., g/mol). – The molar mass of an element is the mass number for the element that we find on the periodic table. – The formula weight (in amu’s) will be the same number as the molar mass (in g/mol). Stoichiometry © 2012 Pearson Education, Inc. ...
Exam Review
... 11. Know how to use the solubility chart to determine if a precipitate forms or not. 12. Lithium exists as two naturally occurring isotopes: Li7 and Li-6. These isotopes have atomic masses 7.015 u and 6.015 u respectively. The average atomic mass of lithium is 6.941 u. Calculate the relative abundan ...
... 11. Know how to use the solubility chart to determine if a precipitate forms or not. 12. Lithium exists as two naturally occurring isotopes: Li7 and Li-6. These isotopes have atomic masses 7.015 u and 6.015 u respectively. The average atomic mass of lithium is 6.941 u. Calculate the relative abundan ...
Slide 1
... Law of Definite Proportions A given compound contains the same elements in exactly the same proportions by mass, regardless of the size of the sample or the source of the compound e.g. NaCl always contains 39.34% by mass of sodium and 60.66% by mass of Chlorine ...
... Law of Definite Proportions A given compound contains the same elements in exactly the same proportions by mass, regardless of the size of the sample or the source of the compound e.g. NaCl always contains 39.34% by mass of sodium and 60.66% by mass of Chlorine ...
Honors Chemistry Unit 4 Student Packet: Honors Chemistry Problem
... 1. The coefficients in a balanced chemical equation can be used to form mole ratios relating reactants to products. 2. To convert molecules to grams you can either use molar mass or Avogadro’s number. 3. One mole of any gas occupies a volume of 22.4L. 4. Mass and the number of moles are conserved in ...
... 1. The coefficients in a balanced chemical equation can be used to form mole ratios relating reactants to products. 2. To convert molecules to grams you can either use molar mass or Avogadro’s number. 3. One mole of any gas occupies a volume of 22.4L. 4. Mass and the number of moles are conserved in ...
Semester Exam Review
... H2(g) + I2(g) 2 HI(g) For the exothermic reaction represented above, carried out at 298K, the rate law is as follows. Rate = k[H2][I2] Predict the effect of each of the following changes on the initial rate of the reaction and explain your prediction. (i) Addition of hydrogen gas at constant tempe ...
... H2(g) + I2(g) 2 HI(g) For the exothermic reaction represented above, carried out at 298K, the rate law is as follows. Rate = k[H2][I2] Predict the effect of each of the following changes on the initial rate of the reaction and explain your prediction. (i) Addition of hydrogen gas at constant tempe ...
Unit A Remediation Review
... 12. What are five clues that will allow you to conclude that a chemical change has occurred? 13. Describe what occurs in the following reaction types, the general equation and an example for each: a) Formation b) Decomposition c) Single Replacement d) Double Replacement e) Combustion 14. Write a bal ...
... 12. What are five clues that will allow you to conclude that a chemical change has occurred? 13. Describe what occurs in the following reaction types, the general equation and an example for each: a) Formation b) Decomposition c) Single Replacement d) Double Replacement e) Combustion 14. Write a bal ...
Rates of Reaction: Chemical Kinetics 50
... A. break the bonds between the reacting molecules B. convert the reactants into the activated complex C. make the reacting particles collide D. form the bonds between the product molecules ...
... A. break the bonds between the reacting molecules B. convert the reactants into the activated complex C. make the reacting particles collide D. form the bonds between the product molecules ...
Types of Chemical Reactions
... Chemical Reactions • Key Concept 2: The process by which one or more substances are rearranged to form different substances is called a chemical reaction. What are some examples of evidence of a chemical reaction? ...
... Chemical Reactions • Key Concept 2: The process by which one or more substances are rearranged to form different substances is called a chemical reaction. What are some examples of evidence of a chemical reaction? ...
chapters 1-4
... Periodic table: symbol, atomic number; elements organized in groups (e.g. noble gases, noble metals) Diatomic molecules exist as natural state of seven elements (all nonmetals). ...
... Periodic table: symbol, atomic number; elements organized in groups (e.g. noble gases, noble metals) Diatomic molecules exist as natural state of seven elements (all nonmetals). ...
L1 – CHEMISTRY FINAL REVIEW
... capillary action; high specific heat (it takes a lot of energy to raise the temperature of water); only substance in which the solid state is less dense than the liquid state; unusually high BP when compared to other molecular compounds with similar molecular weight. 34. How is a saturation point an ...
... capillary action; high specific heat (it takes a lot of energy to raise the temperature of water); only substance in which the solid state is less dense than the liquid state; unusually high BP when compared to other molecular compounds with similar molecular weight. 34. How is a saturation point an ...
Chemistry 2nd Semester Final Review
... CO2(g) + CaO(s). How many grams of calcium carbonate will I need to form 3.45 liters of carbon dioxide? 8. How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of 12.4 atm and a temperature of 85C? 9. How many liters of water can be made from 34 g ...
... CO2(g) + CaO(s). How many grams of calcium carbonate will I need to form 3.45 liters of carbon dioxide? 8. How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of 12.4 atm and a temperature of 85C? 9. How many liters of water can be made from 34 g ...
Investigating Chemistry - Chemistry at Winthrop University
... 4.8 THE MATH OF CHEMICAL REACTIONS: STOICHIOMETRY CALCUATIONS • Stoichiometry uses balanced chemical equations to quantify the masses of reactants and products for a given reaction. • Consider the reaction involved in a natural gas explosion: CH4 + O2 CO2 + H2O • Notice that there is more H on th ...
... 4.8 THE MATH OF CHEMICAL REACTIONS: STOICHIOMETRY CALCUATIONS • Stoichiometry uses balanced chemical equations to quantify the masses of reactants and products for a given reaction. • Consider the reaction involved in a natural gas explosion: CH4 + O2 CO2 + H2O • Notice that there is more H on th ...
chp0-Intro
... • Reactions do not always proceed completely from reactants to products • Chemical equilibrium rates of forward and reverse reaction are equal e.g. ...
... • Reactions do not always proceed completely from reactants to products • Chemical equilibrium rates of forward and reverse reaction are equal e.g. ...
CHAPTER 4 | Solution Chemistry and the Hydrosphere
... The net ionic equations are Cd2+(aq) + 2 OH–(aq) Cd(OH)2(s) Cr3+(aq) + 3 OH–(aq) Cr(OH)3(s) Think about It It is important in the net ionic equation to specify the precipitate as (s). If (aq) is used after the formula for a salt, it implies that the salt is soluble. 4.74. Collect and Organize Si ...
... The net ionic equations are Cd2+(aq) + 2 OH–(aq) Cd(OH)2(s) Cr3+(aq) + 3 OH–(aq) Cr(OH)3(s) Think about It It is important in the net ionic equation to specify the precipitate as (s). If (aq) is used after the formula for a salt, it implies that the salt is soluble. 4.74. Collect and Organize Si ...
Answers for Review Questions Exam 3
... 9. Electrolysis is the use of an electric current to bring about a chemical change. Reduction and oxidation both occur at the same place as in a galvanic cell, but they have different polarities, - and + respectively. It differs from a galvanic cell in that it is in the opposite direction of a galva ...
... 9. Electrolysis is the use of an electric current to bring about a chemical change. Reduction and oxidation both occur at the same place as in a galvanic cell, but they have different polarities, - and + respectively. It differs from a galvanic cell in that it is in the opposite direction of a galva ...
Name__________________________ Honors Chemistry Final
... 1 . It takes 133 sec for a certain amount of gas x to effuse. It takes 22 sec for the same number of moles of N 2 to effuse. Find molar mass of gas x. ...
... 1 . It takes 133 sec for a certain amount of gas x to effuse. It takes 22 sec for the same number of moles of N 2 to effuse. Find molar mass of gas x. ...
12.3 - heoldduscience
... 2) What mass of calcium oxide is produced when 10g of calcium burns? 2Ca + O2 ...
... 2) What mass of calcium oxide is produced when 10g of calcium burns? 2Ca + O2 ...
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.