Introduction to Chemical Equations
... • You may NOT change any subscripts in any of the reactant’s or product’s formulas ...
... • You may NOT change any subscripts in any of the reactant’s or product’s formulas ...
CH 115 Exam 2 - UAB General Chemistry Supplemental Instruction
... Assume the chemical equations on this exam are NOT balanced unless stated otherwise. 1. Balance the equation and give the stoichiometric coefficient for HCl ...
... Assume the chemical equations on this exam are NOT balanced unless stated otherwise. 1. Balance the equation and give the stoichiometric coefficient for HCl ...
PowerPoint
... and the isobaric water-gas shift reaction proceeds to equilibrium, what is the CO conversion if the temperature is (a) 150 °C, (b) 250 °C and (c) 350 °C? ‣ Noting that the water-gas shift reaction is exothermic; predict whether the equilibrium conversion will increase or decrease as the temperature ...
... and the isobaric water-gas shift reaction proceeds to equilibrium, what is the CO conversion if the temperature is (a) 150 °C, (b) 250 °C and (c) 350 °C? ‣ Noting that the water-gas shift reaction is exothermic; predict whether the equilibrium conversion will increase or decrease as the temperature ...
4. Sodium nitrite (NaNO2) is a controversial food preservative added
... 10. A gaseous mixture containing 7.50 mol H2(g) and 9.00 mol Cl2(g) reacts to form hydrogen chloride (HCl) gas. a) Write a balanced equation for the reaction. b) Which reactant is limiting? c) If all the limiting reactant is consumed, how many moles of hydrogen chloride are formed? d) How many moles ...
... 10. A gaseous mixture containing 7.50 mol H2(g) and 9.00 mol Cl2(g) reacts to form hydrogen chloride (HCl) gas. a) Write a balanced equation for the reaction. b) Which reactant is limiting? c) If all the limiting reactant is consumed, how many moles of hydrogen chloride are formed? d) How many moles ...
Section 2-4 “Chemical Reactions and Enzymes”
... reaction started. Once the bonds are broken, the atoms are freed up and can make new molecules. When bonds form between the atoms to make new molecules, energy is released. The specific amount of energy that is needed to break a bond, or is releases when that same bond forms, is called bond energy. ...
... reaction started. Once the bonds are broken, the atoms are freed up and can make new molecules. When bonds form between the atoms to make new molecules, energy is released. The specific amount of energy that is needed to break a bond, or is releases when that same bond forms, is called bond energy. ...
Chemical Reactions & Balancing Equations
... – same number of atoms of each type of element on each side What if it isn’t balanced already? ...
... – same number of atoms of each type of element on each side What if it isn’t balanced already? ...
Notes 2 Balancing
... reactants and in the products, and record the results in a table. • Identify elements that appear in only one reactant and in only one product, and balance the atoms of those elements first. Delay the balancing of atoms (often hydrogen and oxygen) that appear in more that one reactant or product. • ...
... reactants and in the products, and record the results in a table. • Identify elements that appear in only one reactant and in only one product, and balance the atoms of those elements first. Delay the balancing of atoms (often hydrogen and oxygen) that appear in more that one reactant or product. • ...
Problem Set: Empirical and Molecular Formulas
... 6. Titanium (IV) oxide, TiO2, is used as a pigment in paints and as a whitening and coating agent for paper. It can be made by reacting O2 with TiCl4. TiCl4 + O2 TiO2 + 2 Cl2 (already balanced) a) If 4.5 mol of TiCl4 react with 3.5 mol O2, identify both the limiting and excess ...
... 6. Titanium (IV) oxide, TiO2, is used as a pigment in paints and as a whitening and coating agent for paper. It can be made by reacting O2 with TiCl4. TiCl4 + O2 TiO2 + 2 Cl2 (already balanced) a) If 4.5 mol of TiCl4 react with 3.5 mol O2, identify both the limiting and excess ...
Classifying Chemical Reactions 9-3
... A chemical change is really a chemical reaction Has two parts: • Reactants: the substances you start with • Products: the substances you end up with ...
... A chemical change is really a chemical reaction Has two parts: • Reactants: the substances you start with • Products: the substances you end up with ...
Chemical Equations and Tests for anions
... Law of Conservation of Mass The total mass of the products of a chemical reaction is the same as the total mass of the reactants For example if 12 grams of Carbon dioxide react with 32 grams of oxygen 44 grams of carbon dioxide will be formed ...
... Law of Conservation of Mass The total mass of the products of a chemical reaction is the same as the total mass of the reactants For example if 12 grams of Carbon dioxide react with 32 grams of oxygen 44 grams of carbon dioxide will be formed ...
Chapter 1
... The coefficients in a balanced chemical equation give the relative numbers of molecules (or formula units) involved in the reaction. The stoichiometric coefficients in the balanced equation may be interpreted as: • the relative numbers of molecules or formula units involved in the reaction or • the ...
... The coefficients in a balanced chemical equation give the relative numbers of molecules (or formula units) involved in the reaction. The stoichiometric coefficients in the balanced equation may be interpreted as: • the relative numbers of molecules or formula units involved in the reaction or • the ...
673 lab three
... A) DISCUSS CHEMICAL REACTIONS: start with a definition and apply the law of conservation of mass in a chemical reaction to the reaction in this lab. Discuss balanced reactions and give three example reactions and SHOW that they are balanced. Clearly indicate the role of COEFFICIENTS., B) DISCUSS CHE ...
... A) DISCUSS CHEMICAL REACTIONS: start with a definition and apply the law of conservation of mass in a chemical reaction to the reaction in this lab. Discuss balanced reactions and give three example reactions and SHOW that they are balanced. Clearly indicate the role of COEFFICIENTS., B) DISCUSS CHE ...
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and
... 3.6 Quantitative Information from Balanced Equations • Coefficients in balanced chemical equation give relative numbers of molecules (or formula units) involved in the reaction • Stoichiometric coefficients in balanced equation be interpreted as: •relative numbers of molecules or formula units invol ...
... 3.6 Quantitative Information from Balanced Equations • Coefficients in balanced chemical equation give relative numbers of molecules (or formula units) involved in the reaction • Stoichiometric coefficients in balanced equation be interpreted as: •relative numbers of molecules or formula units invol ...
standard sample test
... (a) The solution was found to be acidic. (b) The solution was found to be basic. (c) The solution was found to be neither acidic nor basic, it was neutral. (d) The problem does not have enough information to determine if the solution was found to be acidic, basic or neutral. ...
... (a) The solution was found to be acidic. (b) The solution was found to be basic. (c) The solution was found to be neither acidic nor basic, it was neutral. (d) The problem does not have enough information to determine if the solution was found to be acidic, basic or neutral. ...
Balancing Chemical Equations
... due to the Law of Conservation of Mass, mass of reactants = mass of products o we cannot change the formulas therefore we must change the number of molecules o we do this by adding coefficients in front of the formulas coefficient = number written in front to the chemical symbol or formula balance ...
... due to the Law of Conservation of Mass, mass of reactants = mass of products o we cannot change the formulas therefore we must change the number of molecules o we do this by adding coefficients in front of the formulas coefficient = number written in front to the chemical symbol or formula balance ...
Note Sheet
... Starting with mass percentages, assume you have 100 g of the substance Convert grams of each element to moles Divide each number from #2 by the smallest of those from #2 Check to see if all the numbers are close to integer values-multiply through by a whole number to fix This is your EMPIRICAL FORMU ...
... Starting with mass percentages, assume you have 100 g of the substance Convert grams of each element to moles Divide each number from #2 by the smallest of those from #2 Check to see if all the numbers are close to integer values-multiply through by a whole number to fix This is your EMPIRICAL FORMU ...
one
... – Start by balancing an element that appears in only one reactant and product. – Once one element is balanced, proceed to balance another, and another, until all elements are balanced. – Balance chemical formulas by placing coefficients in front of them. Do not add subscripts, because this will chan ...
... – Start by balancing an element that appears in only one reactant and product. – Once one element is balanced, proceed to balance another, and another, until all elements are balanced. – Balance chemical formulas by placing coefficients in front of them. Do not add subscripts, because this will chan ...
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.