Measurements/Unit Cancellation/Significant Figures 1. When
... Formula mass: The sum of the atomic masses (atomic weights in amu) of the atomic species as given in the formula of the compound Hydrate: A compound in which a specific number of water molecules are associated with each formula unit. Hydrated ion: An ion in which a specific number of water molecules ...
... Formula mass: The sum of the atomic masses (atomic weights in amu) of the atomic species as given in the formula of the compound Hydrate: A compound in which a specific number of water molecules are associated with each formula unit. Hydrated ion: An ion in which a specific number of water molecules ...
03. The Theoretic bases of bioenergetics
... may be altered (converted), but not created (from nothingness) nor destroyed (reduced to nothingness). The First Law teaches that matter/energy cannot spring forth from nothing without cause, nor can it simply vanish. Energy can neither be created nor destroyed although it may be converted from on ...
... may be altered (converted), but not created (from nothingness) nor destroyed (reduced to nothingness). The First Law teaches that matter/energy cannot spring forth from nothing without cause, nor can it simply vanish. Energy can neither be created nor destroyed although it may be converted from on ...
Ch 2-1 Properties of Matter
... 72) The wax appears to disappear because the products of the reaction—carbon dioxide and water vapor—are colorless. 79) a) yes; because the graph is a straight line, the proportion of iron to oxygen is a constant, which is true for a compound. b) no; a point for the values given wouldn’t fall on the ...
... 72) The wax appears to disappear because the products of the reaction—carbon dioxide and water vapor—are colorless. 79) a) yes; because the graph is a straight line, the proportion of iron to oxygen is a constant, which is true for a compound. b) no; a point for the values given wouldn’t fall on the ...
Name ______ Period ______ 7th Grade Science Study Guide 1 7
... 52. Which of the following summarizes the Law of Conservation of Matter as applied to a chemical reaction? a. The total mass of the reactants is greater than the mass of the products. b. The total mass of the reactants is less than the total mass of the products. c. The total mass of the reactants e ...
... 52. Which of the following summarizes the Law of Conservation of Matter as applied to a chemical reaction? a. The total mass of the reactants is greater than the mass of the products. b. The total mass of the reactants is less than the total mass of the products. c. The total mass of the reactants e ...
Free Energy I
... constant P) would decrease the entropy of the system by 326.3 J/K for every mole of O2 or every two moles of water or H2. How much does the entropy change when 0.275 g of H2 is ignited with O2 in a constant-pressure system? 0.275 g H2(g) 1 mol H2 ...
... constant P) would decrease the entropy of the system by 326.3 J/K for every mole of O2 or every two moles of water or H2. How much does the entropy change when 0.275 g of H2 is ignited with O2 in a constant-pressure system? 0.275 g H2(g) 1 mol H2 ...
Document
... 10. How many Chlorine atoms are present in the compound Ca(ClO3)2? 11. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2? 12. What is the name of the compound with the formula NaCl? 13. Why do the noble gases NOT form compounds readily? 14. In a chemical formula, the ...
... 10. How many Chlorine atoms are present in the compound Ca(ClO3)2? 11. How many hydrogen atoms are present in one molecule of ammonium acetate, NH4C2H3O2? 12. What is the name of the compound with the formula NaCl? 13. Why do the noble gases NOT form compounds readily? 14. In a chemical formula, the ...
General Chemistry First Semester Review General
... Phase notations (solid, liquids, gases, aqueous) - aqueous (aq) is written if a solution is used - pure liquids (not a mixture of something) use (l) - solid: This could refer to a multitude of different substances: metals, flakes, crystals, and precipitates; use (s) - gas: Use (g), these are usually ...
... Phase notations (solid, liquids, gases, aqueous) - aqueous (aq) is written if a solution is used - pure liquids (not a mixture of something) use (l) - solid: This could refer to a multitude of different substances: metals, flakes, crystals, and precipitates; use (s) - gas: Use (g), these are usually ...
11-1 SECTION 11 THERMOCHEMISTRY Thermochemistry: Study of
... implies that when 2 moles of gaseous dihydrogen reacts with one mole of gaseous dioxygen to give two moles of liquid water 570 kilojoules of energy is released from the reacting system to its surroundings.] The ∆ means change, r stands for reaction and H is the symbol for enthalpy. ∆rH is the enthal ...
... implies that when 2 moles of gaseous dihydrogen reacts with one mole of gaseous dioxygen to give two moles of liquid water 570 kilojoules of energy is released from the reacting system to its surroundings.] The ∆ means change, r stands for reaction and H is the symbol for enthalpy. ∆rH is the enthal ...
AP Chemistry Syllabus 2013 Mawhiney
... course. Analysis of data from AP Chemistry examinees shows that increased laboratory time is correlated with higher AP grades. Depending on the particular lab, students will work individually or collaboratively to physically manipulate equipment and materials in order to make relevant observations a ...
... course. Analysis of data from AP Chemistry examinees shows that increased laboratory time is correlated with higher AP grades. Depending on the particular lab, students will work individually or collaboratively to physically manipulate equipment and materials in order to make relevant observations a ...
Stoichiometry and the mole
... 1. Base calculation on 100 grams of compound. 2. Determine moles of each element in 100 grams of compound. 3. Divide each value of moles by the smallest of the values. 4. Multiply each number by an integer to obtain ...
... 1. Base calculation on 100 grams of compound. 2. Determine moles of each element in 100 grams of compound. 3. Divide each value of moles by the smallest of the values. 4. Multiply each number by an integer to obtain ...
Chemistry Final Exam Review 2006-2007
... 6. How does rate change if you increase the concentration of the reactants? 7. How does rate change if you increase the surface area? 8. How does rate change if you decrease the temperature? 9. How does rate change if you add a catalyst? 10. Write the equilibrium expression for the following reactio ...
... 6. How does rate change if you increase the concentration of the reactants? 7. How does rate change if you increase the surface area? 8. How does rate change if you decrease the temperature? 9. How does rate change if you add a catalyst? 10. Write the equilibrium expression for the following reactio ...
Reactions I Can..
... 3. Calculate molar mass for a compound given the name or formula of that compound 4. Apply significant figures to molar mass values 5. Convert from mass in grams to moles and the reverse (one step conversions). 6. Convert from mass in grams to number of atoms/molecules/ions and the reverse (two step ...
... 3. Calculate molar mass for a compound given the name or formula of that compound 4. Apply significant figures to molar mass values 5. Convert from mass in grams to moles and the reverse (one step conversions). 6. Convert from mass in grams to number of atoms/molecules/ions and the reverse (two step ...
Atoms
... 1. Correctly name a chemical compound when given a chemical formula from the following categories: binary & ternary ionic, binary & ternary acids, and binary non-organic molecules. 2. Correctly write the chemical formula when given the name of the chemical from the following categories: binary & ter ...
... 1. Correctly name a chemical compound when given a chemical formula from the following categories: binary & ternary ionic, binary & ternary acids, and binary non-organic molecules. 2. Correctly write the chemical formula when given the name of the chemical from the following categories: binary & ter ...
chemical reaction
... those of Ag+, Hg+ & Pb+2 4. All sulfates are soluble except: Ba+2, Sr+2, Ca+2, Pb+2,Ag+, ...
... those of Ag+, Hg+ & Pb+2 4. All sulfates are soluble except: Ba+2, Sr+2, Ca+2, Pb+2,Ag+, ...
Measuring and Calculating
... Because gases have more ranges of motion than liquids and solids, at constant temperature gases tend to have more entropy followed by liquids and solids example: An ice cube is placed on a hot skillet. 1st as it melts the entropy increases, 2nd as the liquid evaporates the entropy increases furt ...
... Because gases have more ranges of motion than liquids and solids, at constant temperature gases tend to have more entropy followed by liquids and solids example: An ice cube is placed on a hot skillet. 1st as it melts the entropy increases, 2nd as the liquid evaporates the entropy increases furt ...
C. - Knights of The Periodic Table
... A. 2HCl + 2NaOH → Na(OH)2 + H2Cl2 B. HCl2 + 2Na(OH)2 → 2H2O +2NaCl + OH C. HCl + NaOH → H2O + NaCl D. 2HCl + Na(OH)2 → 2H2 + NaCl + O2 ...
... A. 2HCl + 2NaOH → Na(OH)2 + H2Cl2 B. HCl2 + 2Na(OH)2 → 2H2O +2NaCl + OH C. HCl + NaOH → H2O + NaCl D. 2HCl + Na(OH)2 → 2H2 + NaCl + O2 ...
Document
... d) carbon tetrafluoride e) calcium chloride f) sodium hydroxide 43. Predict the products and write a balanced chemical equation for the following chemical reactions: a) Copper wire is added to an aqueous solution of silver nitrate. (3 marks) b) Potassium metal is added to water. (3 marks) c) Butane, ...
... d) carbon tetrafluoride e) calcium chloride f) sodium hydroxide 43. Predict the products and write a balanced chemical equation for the following chemical reactions: a) Copper wire is added to an aqueous solution of silver nitrate. (3 marks) b) Potassium metal is added to water. (3 marks) c) Butane, ...
Pb2+ +2I- → PbI2 (s)
... What is happened to the molecule when you are changing the state of matter? Breaking intermolecular attractions, NOT the bonds. ...
... What is happened to the molecule when you are changing the state of matter? Breaking intermolecular attractions, NOT the bonds. ...
Chemistry Final Exam Review 2006-2007
... metal has a mass of 25 g and had a temperature change of 5C. b) How much heat is released when iron is dropped in a beaker of water. The mass of the metal was 43 g and the initial temperature of the metal was 78 C. The water temperature changed from 25 C to 32 C. The specific heat of the metal is .4 ...
... metal has a mass of 25 g and had a temperature change of 5C. b) How much heat is released when iron is dropped in a beaker of water. The mass of the metal was 43 g and the initial temperature of the metal was 78 C. The water temperature changed from 25 C to 32 C. The specific heat of the metal is .4 ...
+ H 2
... • the most reactive metal ends up as an ion and then reacts to form a new compound o Zn + CuSO4 Cu + ZnSO4 • Zn is more reactive than Cu • Zn is oxidized (goes from 0 to +2) and then bonds with the -2 SO4 o Ni + 2AgNO3 2Ag + Ni(NO3)2 • Ni is more reactive that Ag • Ni is oxidized (goes from 0 ...
... • the most reactive metal ends up as an ion and then reacts to form a new compound o Zn + CuSO4 Cu + ZnSO4 • Zn is more reactive than Cu • Zn is oxidized (goes from 0 to +2) and then bonds with the -2 SO4 o Ni + 2AgNO3 2Ag + Ni(NO3)2 • Ni is more reactive that Ag • Ni is oxidized (goes from 0 ...
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.