Midterm Review File
... 44. If the empirical formula is CO2 and the molecular mass is 176.0 g/mol. What is its molecular formula? ...
... 44. If the empirical formula is CO2 and the molecular mass is 176.0 g/mol. What is its molecular formula? ...
Reaction Rates
... the amount of reactant present at the start of the reaction the speed of the reaction the amount of product produced from the reaction How concentrated the reactants are ...
... the amount of reactant present at the start of the reaction the speed of the reaction the amount of product produced from the reaction How concentrated the reactants are ...
Introductory Chemistry: A Foundation Introductory Chemistry Basic
... reactants and products (include physical states). • Balance the equation by counting the atoms on both sides of the equation and changing the coefficients as needed. Never change the subscripts! • This is done by trial and error. Start with the most ...
... reactants and products (include physical states). • Balance the equation by counting the atoms on both sides of the equation and changing the coefficients as needed. Never change the subscripts! • This is done by trial and error. Start with the most ...
Honors Chemistry
... Where are the 3 different types of bonds? What are the differences between them? How is the bond determined to be any of the three? What type of bond is present in CaCl2, CO2, SO2 and NH3? What is the difference between a polar and a nonpolar molecule? Give an example of each. 5. What are the differ ...
... Where are the 3 different types of bonds? What are the differences between them? How is the bond determined to be any of the three? What type of bond is present in CaCl2, CO2, SO2 and NH3? What is the difference between a polar and a nonpolar molecule? Give an example of each. 5. What are the differ ...
Chapter 11 Chemical Reactions
... Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. HNO3 (aq) + Na2CO3 (s) ...
... Nitric acid dissolved in water reacts with solid sodium carbonate to form liquid water and carbon dioxide gas and sodium nitrate dissolved in water. HNO3 (aq) + Na2CO3 (s) ...
Stoichiometry
... How many moles of hydrogen are produced when 0.0400 mole of potassium is used? 2K + 2H20 2KOH + H2 1. Identify the known… K 2. Identify the unknown…H2 3. To solve this problem, you need to know how the unknown moles of H2 are related to the know moles of K 4. The correct ratio should have the mol ...
... How many moles of hydrogen are produced when 0.0400 mole of potassium is used? 2K + 2H20 2KOH + H2 1. Identify the known… K 2. Identify the unknown…H2 3. To solve this problem, you need to know how the unknown moles of H2 are related to the know moles of K 4. The correct ratio should have the mol ...
Chapter #2-Newest CPub
... does not change during a chemical reaction (Lavoisier). • Law of Definite (or Constant) Composition: No matter what its source, a particular chemical compound is composed of the same elements in the same parts (fractions) by mass (Proust). • The Law of Multiple Proportions: When two elements form a ...
... does not change during a chemical reaction (Lavoisier). • Law of Definite (or Constant) Composition: No matter what its source, a particular chemical compound is composed of the same elements in the same parts (fractions) by mass (Proust). • The Law of Multiple Proportions: When two elements form a ...
Practice problem chap3 1. The atomic mass of 35Cl (75.53%) and
... 1. The atomic mass of Cl (75.53%) and 37Cl (24.47%) are 34.968amu and 36.956amu.Calculate the average atomic mass in amu. 2. What is the mass percent (%) for O in SO2? (a) 38.09 (b) 45.41 (c) 50.00 (d) 53.86 (e) 56.43 3. How many molecules of ethane (C2H6) are present in 0.334g of C2H6?How many H at ...
... 1. The atomic mass of Cl (75.53%) and 37Cl (24.47%) are 34.968amu and 36.956amu.Calculate the average atomic mass in amu. 2. What is the mass percent (%) for O in SO2? (a) 38.09 (b) 45.41 (c) 50.00 (d) 53.86 (e) 56.43 3. How many molecules of ethane (C2H6) are present in 0.334g of C2H6?How many H at ...
1. What is a Chemical Reaction?
... • A chemical reaction is the process by which atoms of one or more substances are rearranged to form different substances(s) with new chemical and physical properties. • A chemical reaction is another name for a chemical change. • When substances chemically react, observations can be made that provi ...
... • A chemical reaction is the process by which atoms of one or more substances are rearranged to form different substances(s) with new chemical and physical properties. • A chemical reaction is another name for a chemical change. • When substances chemically react, observations can be made that provi ...
unit 7 – writing and balancing chemical equations
... (d) copper(II) chloride solution plus aluminum (e) sodium chloride solution plus calcium ...
... (d) copper(II) chloride solution plus aluminum (e) sodium chloride solution plus calcium ...
Practice Toxins Mid-Unit Test 08-09
... ______1. What type of reaction is this? Ag (s) + CuI2 (aq) AgI (s) + Cu(s) (A) single displacement (B) double displacement (C) combination reaction (D) decomposition reaction ______2.Calcium Chloride is abbreviated (A) CaCl (C) Ca2Cl (B) CaCl2 (D) Cl2Ca ______3. What is the molarity of 3.5 moles o ...
... ______1. What type of reaction is this? Ag (s) + CuI2 (aq) AgI (s) + Cu(s) (A) single displacement (B) double displacement (C) combination reaction (D) decomposition reaction ______2.Calcium Chloride is abbreviated (A) CaCl (C) Ca2Cl (B) CaCl2 (D) Cl2Ca ______3. What is the molarity of 3.5 moles o ...
Date Hour
... Aqueous solution (a metal salt dissolved in water or an acid or base). The word solution is your clue that you are to use the subscript (aq). ...
... Aqueous solution (a metal salt dissolved in water or an acid or base). The word solution is your clue that you are to use the subscript (aq). ...
4 - Ms McRae`s Science
... a)yes bec an increase in the temperature of the HCl will increase the velocity of the reactant particles which will increase the number of collisions AND increase the number of effective collisions i.e. ones that have sufficient energy (activation energy) to react b) skipping this one for now until ...
... a)yes bec an increase in the temperature of the HCl will increase the velocity of the reactant particles which will increase the number of collisions AND increase the number of effective collisions i.e. ones that have sufficient energy (activation energy) to react b) skipping this one for now until ...
Chapter 3 - pennsaukenchemistry2
... NO2. The colourless liquid, used in rocket engines has a molar mass of 92.0 g/mole. What is the molecular formula of this ...
... NO2. The colourless liquid, used in rocket engines has a molar mass of 92.0 g/mole. What is the molecular formula of this ...
Slide 1
... EXAMPLE: If the empirical formula is CH2O and the molecular mass is 90 g/mole, what is the molecular formula. WE KNOW THE MOLECULAR FORMULA IS SOME WHOLE NUMBER MULTIPLE OF THE EMPIRICAL FORMULA, SO CALCULATE THE EMPIRICAL MASS 1C + 2H + 1O = 12 + 2 + 16 = 30 DIVIDE 90 BY 30 = 90/30 = 3, SO MOLECULA ...
... EXAMPLE: If the empirical formula is CH2O and the molecular mass is 90 g/mole, what is the molecular formula. WE KNOW THE MOLECULAR FORMULA IS SOME WHOLE NUMBER MULTIPLE OF THE EMPIRICAL FORMULA, SO CALCULATE THE EMPIRICAL MASS 1C + 2H + 1O = 12 + 2 + 16 = 30 DIVIDE 90 BY 30 = 90/30 = 3, SO MOLECULA ...
File
... products are on the right side of the arrow. The mass of the reactants equals 80g and the mass of the products equals 80g (Law of conservation of mass). You should also notice that in CH4 there is one Carbon atom, and four hydrogen atoms (Law of definite proportions). Electrolysis Reactions: Carri ...
... products are on the right side of the arrow. The mass of the reactants equals 80g and the mass of the products equals 80g (Law of conservation of mass). You should also notice that in CH4 there is one Carbon atom, and four hydrogen atoms (Law of definite proportions). Electrolysis Reactions: Carri ...
Critical Thinking Questions 4
... CHEM1001 Worksheet 4: Moles and Stoichiometry Model 1: Balancing Chemical Equations Chemical equations specify how chemical reactions occur – the reactants used, the products formed and the amounts of each. A balanced equation has the same number of atoms of each element on both sides, because matte ...
... CHEM1001 Worksheet 4: Moles and Stoichiometry Model 1: Balancing Chemical Equations Chemical equations specify how chemical reactions occur – the reactants used, the products formed and the amounts of each. A balanced equation has the same number of atoms of each element on both sides, because matte ...
Matter, Mass and Weight
... substance is formed. A chemical change is described by a chemical equation. Formulas of initial substances are written to the left of an arrow that points to the formulas of substances formed or products. For example, the reaction of magnesium and oxygen to form magnesium oxide is 2 Mg + O2 -------- ...
... substance is formed. A chemical change is described by a chemical equation. Formulas of initial substances are written to the left of an arrow that points to the formulas of substances formed or products. For example, the reaction of magnesium and oxygen to form magnesium oxide is 2 Mg + O2 -------- ...
Chapters 6 and 17: Chemical Thermodynamics
... (a) Calculate the molar heat of combustion of phenol in kilojoules per mole at 25°C. (b) Calculate the standard heat of formation, H°f, of phenol in kilojoules per mole at 25°C. (c) Calculate the value of the standard free-energy change, G° for the combustion of phenol at 25°C. (d) If the volume o ...
... (a) Calculate the molar heat of combustion of phenol in kilojoules per mole at 25°C. (b) Calculate the standard heat of formation, H°f, of phenol in kilojoules per mole at 25°C. (c) Calculate the value of the standard free-energy change, G° for the combustion of phenol at 25°C. (d) If the volume o ...
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.