![HS-PS1-2. Construct and revise an explanation for the outcome of a](http://s1.studyres.com/store/data/022113319_1-3e0b59c3555112d40280164e67d90988-300x300.png)
HS-PS1-2. Construct and revise an explanation for the outcome of a
... energy change. Examples of models could include molecular-level drawings and diagrams of reactions, graphs showing the relative energies of reactants and products, and representations showing energy is conserved.] [Assessment Boundary: Assessment does not include calculating the total bond energy ch ...
... energy change. Examples of models could include molecular-level drawings and diagrams of reactions, graphs showing the relative energies of reactants and products, and representations showing energy is conserved.] [Assessment Boundary: Assessment does not include calculating the total bond energy ch ...
Questions for Study
... 10. A 17.9-g sample of an unknown metal was heated to 48.31°C. It was then added to 28.05 g of water in an insulated cup. The water temperature rose from 21.04 to 23.98°C. What is the specific heat of the metal? 11. Ethane gas, C2H6, burns in oxygen to form carbon dioxide gas, CO2, and gaseous water ...
... 10. A 17.9-g sample of an unknown metal was heated to 48.31°C. It was then added to 28.05 g of water in an insulated cup. The water temperature rose from 21.04 to 23.98°C. What is the specific heat of the metal? 11. Ethane gas, C2H6, burns in oxygen to form carbon dioxide gas, CO2, and gaseous water ...
CHEMISTRY PHYSICAL SETTING Thursday, PS/CHEMISTRY
... Record the number of your choice for each Part A and Part B–1 multiple-choice question on your separate answer sheet. Write your answers to the Part B–2 and Part C questions in your answer booklet. All work should be written in pen, except for graphs and drawings, which should be done in pencil. You ...
... Record the number of your choice for each Part A and Part B–1 multiple-choice question on your separate answer sheet. Write your answers to the Part B–2 and Part C questions in your answer booklet. All work should be written in pen, except for graphs and drawings, which should be done in pencil. You ...
K,7th Grade Test Review: Atoms and Chemical Reactions PART
... PART FOUR: Chemical Equations. For each equation, label the products and reactants. Then, count the number of atoms of each element on each side. Then fill in the blanks. ...
... PART FOUR: Chemical Equations. For each equation, label the products and reactants. Then, count the number of atoms of each element on each side. Then fill in the blanks. ...
4.2- Reaction Stoichiometry Reaction Stoichiometry
... on the relationship between mass and moles Such calculations are fundamental to most quantitative work in chemistry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances involved in the reaction ...
... on the relationship between mass and moles Such calculations are fundamental to most quantitative work in chemistry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances involved in the reaction ...
PPT File - Clark Magnet High School
... 4 Al(s) + 3 O2(g) 2 Al2O3(s) 4 moles: 3 moles Look up atomic mass of aluminum 26.98 amu – remember 1 mole is atomic mass in g 107.92 g x 1 mol = 4 mol 26.98g Which is what we need according to the equation ...
... 4 Al(s) + 3 O2(g) 2 Al2O3(s) 4 moles: 3 moles Look up atomic mass of aluminum 26.98 amu – remember 1 mole is atomic mass in g 107.92 g x 1 mol = 4 mol 26.98g Which is what we need according to the equation ...
REACTING MASSES – ACTIVITY SHEET
... 7. 2NH3 (g) + H2SO4 (aq) → (NH4)2SO4(aq) Calculate the volume of ammonia gas that would react with excess sulphuric acid to produce 33g of ammonium sulphate. Take the molar gas volume to be 24 litres mol-1. 8. Zn (s) + 2HCl(aq) → ZnCl2 (aq) + H2 (g) Use the equation above to calculate the volume of ...
... 7. 2NH3 (g) + H2SO4 (aq) → (NH4)2SO4(aq) Calculate the volume of ammonia gas that would react with excess sulphuric acid to produce 33g of ammonium sulphate. Take the molar gas volume to be 24 litres mol-1. 8. Zn (s) + 2HCl(aq) → ZnCl2 (aq) + H2 (g) Use the equation above to calculate the volume of ...
Chapter 2 - profpaz.com
... The law of multiple proportions states that when two elements combine to form two different compounds, the atoms combine in simple, whole-number ratios. ...
... The law of multiple proportions states that when two elements combine to form two different compounds, the atoms combine in simple, whole-number ratios. ...
Chemical Quantities PPT
... atoms or formula units Since atoms are so small, extremely large numbers are needed in calculations Need to use a special counting unit just as used for other items A ream of paper One dozen donuts A pair of shoes ...
... atoms or formula units Since atoms are so small, extremely large numbers are needed in calculations Need to use a special counting unit just as used for other items A ream of paper One dozen donuts A pair of shoes ...
Examples
... The same as: 1) Gram Molecular Mass (for molecules) 2) Gram Formula Mass (ionic compounds) 3) Gram Atomic Mass (for elements) – molar mass is just a much broader term than these other specific masses ...
... The same as: 1) Gram Molecular Mass (for molecules) 2) Gram Formula Mass (ionic compounds) 3) Gram Atomic Mass (for elements) – molar mass is just a much broader term than these other specific masses ...
Calorimetry Notes
... can be written as either a reactant or a product A thermochemical equation includes the enthalpy change The heat of reaction is the enthalpy change for the chemical equation exactly as it is written The heat of combustion is the heat of reaction for the complete burning of one mole of a substa ...
... can be written as either a reactant or a product A thermochemical equation includes the enthalpy change The heat of reaction is the enthalpy change for the chemical equation exactly as it is written The heat of combustion is the heat of reaction for the complete burning of one mole of a substa ...
Key - GCC
... a. Law of Conservation of Mass Matter is neither created nor destroyed in a chemical reaction – molecules change (atoms rearrange) to create new substances. b. Law of Definite Proportions All samples of a given substance will have the same ratio of atoms by mass (e.g., carbon dioxide is always CO2). ...
... a. Law of Conservation of Mass Matter is neither created nor destroyed in a chemical reaction – molecules change (atoms rearrange) to create new substances. b. Law of Definite Proportions All samples of a given substance will have the same ratio of atoms by mass (e.g., carbon dioxide is always CO2). ...
workbook Chem (WP)
... 3. Write the formula for the following: a) hydrochloric acid b) phosphoric acid c) carbonous acid d) hydrofluoric acid e) nitric acid 4. Write the name for each of the following: a) H3N (aq) b) HClO4 (aq) c) HNO2 (aq) d) H2Se (aq) e) C6H5COOH (aq) ...
... 3. Write the formula for the following: a) hydrochloric acid b) phosphoric acid c) carbonous acid d) hydrofluoric acid e) nitric acid 4. Write the name for each of the following: a) H3N (aq) b) HClO4 (aq) c) HNO2 (aq) d) H2Se (aq) e) C6H5COOH (aq) ...
Discover Chemical Changes - gk-12
... in everyday language, only applied to the molecules that make up something. When something decomposes, the molecules that make up that substance are broken up into smaller and smaller pieces and eventually down to atoms, becoming something different that what they were before. Rotting is also associ ...
... in everyday language, only applied to the molecules that make up something. When something decomposes, the molecules that make up that substance are broken up into smaller and smaller pieces and eventually down to atoms, becoming something different that what they were before. Rotting is also associ ...
Chapter 8 and 9 – Energy Balances
... enthalpy of pure component i. If the specific enthalpy is expressed per unit mass, then xi is the mass fraction; if instead Ĥ i is expressed per mole, then xi is the mole fraction. The assumption that a mixture behaves ideally nearly always works well for mixtures of gases, and it also works well f ...
... enthalpy of pure component i. If the specific enthalpy is expressed per unit mass, then xi is the mass fraction; if instead Ĥ i is expressed per mole, then xi is the mole fraction. The assumption that a mixture behaves ideally nearly always works well for mixtures of gases, and it also works well f ...
Unit 13, Lesson 1
... metals are arranged according to their ability to displace hydrogen from an acid or water. Lithium is the most reactive metal, gold is the least reactive. 1. Hydrogen Displacement All alkali metals and some alkaline earth metals will displace hydrogen from cold water. 2Na(s) + H2O(l) 2NaOH(aq) + H ...
... metals are arranged according to their ability to displace hydrogen from an acid or water. Lithium is the most reactive metal, gold is the least reactive. 1. Hydrogen Displacement All alkali metals and some alkaline earth metals will displace hydrogen from cold water. 2Na(s) + H2O(l) 2NaOH(aq) + H ...
The format of this test is MULTIPLE CHOICE
... Generation of heat/cold, light, solid from liquid, smoke, odor 2. Use the word bank to match the correct term with its definition. decomposition reaction Law of Conservation of Mass double replacement reactions neutralization reaction ...
... Generation of heat/cold, light, solid from liquid, smoke, odor 2. Use the word bank to match the correct term with its definition. decomposition reaction Law of Conservation of Mass double replacement reactions neutralization reaction ...
Redox I
... 1-6 (as before) to balance the equation as if it took place in acidic solution. Then perform one more step: Step 7. (ONLY for redox reactions taking place in basic solution!) Add OH- to BOTH sides of the equation to cancel all of the H+, then make sure H2O appears only on one side of the equation. I ...
... 1-6 (as before) to balance the equation as if it took place in acidic solution. Then perform one more step: Step 7. (ONLY for redox reactions taking place in basic solution!) Add OH- to BOTH sides of the equation to cancel all of the H+, then make sure H2O appears only on one side of the equation. I ...
Stoichiometry
![](https://commons.wikimedia.org/wiki/Special:FilePath/Combustion_reaction_of_methane.jpg?width=300)
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.