2 - DrChoChemistryWebSite
... (s) after the formula = solid: Fe(s) (g) after the formula = gas: CO2(g) (l) after the formula = liquid: H2O(l) ...
... (s) after the formula = solid: Fe(s) (g) after the formula = gas: CO2(g) (l) after the formula = liquid: H2O(l) ...
Nature of chemical reaction - Environmental-Chemistry
... in reaction, and reactants are always written at left side of equation. CO2 + 2H2O called products that is formed as a result of reaction and products are always written at right side of equation. ...
... in reaction, and reactants are always written at left side of equation. CO2 + 2H2O called products that is formed as a result of reaction and products are always written at right side of equation. ...
Using mass to calculate molecular formula
... Chemical Reactions and Chemical Equations Compounds react to form other compounds – chemical reactions. Reactions are described by a chemical equation. e.g. ...
... Chemical Reactions and Chemical Equations Compounds react to form other compounds – chemical reactions. Reactions are described by a chemical equation. e.g. ...
Stoichiometry: Calculations with Chemical Formulas and
... Avogadro’s number of those particles • One mole of molecules or formula units contains Avogadro’s number times the number of atoms or ions of each element in the compound Stoichiometry ...
... Avogadro’s number of those particles • One mole of molecules or formula units contains Avogadro’s number times the number of atoms or ions of each element in the compound Stoichiometry ...
Kinetics & Equilibrium
... Hcomb = HEAT ABSORBED WHEN 1 MOLE OF A SUBSTANCE REACTS WITH OXYGEN AT CONSTANT P ...
... Hcomb = HEAT ABSORBED WHEN 1 MOLE OF A SUBSTANCE REACTS WITH OXYGEN AT CONSTANT P ...
File
... 3. __________________: When two or more elements combine chemically you get a mixture. 4. __________________: The properties of elements do not change when mixtures are formed. 5. __________________: Particles in a solid are not packed at all. 6. __________________: Solids keep their shape. 7. _____ ...
... 3. __________________: When two or more elements combine chemically you get a mixture. 4. __________________: The properties of elements do not change when mixtures are formed. 5. __________________: Particles in a solid are not packed at all. 6. __________________: Solids keep their shape. 7. _____ ...
Introduction to Chemical Equations
... using the names of the reactants and products. Write the word equation for the reaction of methane gas with oxygen gas to form carbon dioxide and water. ...
... using the names of the reactants and products. Write the word equation for the reaction of methane gas with oxygen gas to form carbon dioxide and water. ...
Single-Replacement Reactions
... • If you change the formula you are describing a different reaction. • H2O is a different compound than H2O2 ...
... • If you change the formula you are describing a different reaction. • H2O is a different compound than H2O2 ...
Exam 2-f06 - Clayton State University
... Exams will be picked up at the end of the class period. No late exams will be accepted! You are allowed to use a calculator. If you do not have a calculator, setting up the problem correctly will gain you some points but you will not receive full credit for any ...
... Exams will be picked up at the end of the class period. No late exams will be accepted! You are allowed to use a calculator. If you do not have a calculator, setting up the problem correctly will gain you some points but you will not receive full credit for any ...
Chemistry Standards Review
... 28. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 29. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 + CO b. C4H10 + O2 CO2 + H2O c. P + O2 P2O5 30. What isotope i ...
... 28. Why do the atoms and molecules in liquids move in a random pattern relative to one another instead of being in a solid form? Conservation of Matter and Stoichiometry 29. Balance the following equations: a. Al2O3 + Cl2 + C AlCl3 + CO b. C4H10 + O2 CO2 + H2O c. P + O2 P2O5 30. What isotope i ...
Properties of Metals vs. Nonmetals vs. Metalloids
... Lead (II) hydroxide __________________________ chromium (III) sulfate ___________________ ...
... Lead (II) hydroxide __________________________ chromium (III) sulfate ___________________ ...
Properties of Metals vs. Nonmetals vs. Metalloids
... Lead (II) hydroxide __________________________ chromium (III) sulfate ___________________ ...
... Lead (II) hydroxide __________________________ chromium (III) sulfate ___________________ ...
stoichiometry power point File
... all identical for the purposes of weighing (refer to the jelly bean example on p. 77-78). • Since atoms are small it makes more sense to count them by mass than by getting out our ...
... all identical for the purposes of weighing (refer to the jelly bean example on p. 77-78). • Since atoms are small it makes more sense to count them by mass than by getting out our ...
Chemical Reactions
... Convert moles to grams Convert grams to moles Convert atoms/molecules to moles Convert moles to atoms/molecules Find the empirical and molecular formula of a compound Find the percent composition of a compound Find a mole ratio Convert moles/grams of a substance to moles/grams of a different substan ...
... Convert moles to grams Convert grams to moles Convert atoms/molecules to moles Convert moles to atoms/molecules Find the empirical and molecular formula of a compound Find the percent composition of a compound Find a mole ratio Convert moles/grams of a substance to moles/grams of a different substan ...
Chemistry PowerPoint
... c. The total mass of the reactants equals the total mass of the products d. Mass can be created and destroyed ...
... c. The total mass of the reactants equals the total mass of the products d. Mass can be created and destroyed ...
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.