Determining Chemical Formulas
... temperature contain equal numbers of molecules Leads to definition of the “mole” Mole Def: the number equal to the number of atoms in 12.01 grams of carbon ...
... temperature contain equal numbers of molecules Leads to definition of the “mole” Mole Def: the number equal to the number of atoms in 12.01 grams of carbon ...
Stoichiometry Objectives
... -we round Avogadro’s number to three significant figures— 6.02 x 1023. - If you write out Avogadro’s number, it looks like this: ...
... -we round Avogadro’s number to three significant figures— 6.02 x 1023. - If you write out Avogadro’s number, it looks like this: ...
Chemical Thermodynamics (with Thermochemistry) Addresses the
... EX 6. 0.1584 g of benzoic acid (C6H5COOH) are combusted in a constant volume bomb calorimeter. The temperature of the calorimeter rises by 2.54°C. ΔE for the combustion of benzoic acid is -26.38 kJ g-1. Determine the heat capacity of the calorimeter. ...
... EX 6. 0.1584 g of benzoic acid (C6H5COOH) are combusted in a constant volume bomb calorimeter. The temperature of the calorimeter rises by 2.54°C. ΔE for the combustion of benzoic acid is -26.38 kJ g-1. Determine the heat capacity of the calorimeter. ...
iClicker PARTICIPATION Question: Development of the Modern
... Development of the Modern Atomic Theory In 1803, John Dalton proposed an atomic theory that is still the basis for many of our theories about the atom. 1. All matter is composed of atoms, which are tiny, indivisible particles. 2. A chemical reaction is a rearrangement of atoms to form different comp ...
... Development of the Modern Atomic Theory In 1803, John Dalton proposed an atomic theory that is still the basis for many of our theories about the atom. 1. All matter is composed of atoms, which are tiny, indivisible particles. 2. A chemical reaction is a rearrangement of atoms to form different comp ...
Mass Relationships in Chemical Reactions
... with both % Composition and Molar Mass A sample of a compound contains 30.46% Nitrogen and 69.54% Oxygen by mass In a separate experiment, the molar mass of the compound is estimated to be between 90 g and 95 g. Determine the molecular formula and the accurate molar mass of the compound. ...
... with both % Composition and Molar Mass A sample of a compound contains 30.46% Nitrogen and 69.54% Oxygen by mass In a separate experiment, the molar mass of the compound is estimated to be between 90 g and 95 g. Determine the molecular formula and the accurate molar mass of the compound. ...
Midterm Review Answers
... solutions with sodium chloride would mean that only one solution would result in precipitate, which is the mercury solution. To distinguish between barium and magnesium ions, react with sodium hydroxide. Magnesium is insoluble (precipitate will form) in hydroxides whereas barium is soluble, so which ...
... solutions with sodium chloride would mean that only one solution would result in precipitate, which is the mercury solution. To distinguish between barium and magnesium ions, react with sodium hydroxide. Magnesium is insoluble (precipitate will form) in hydroxides whereas barium is soluble, so which ...
1-Three states of matter . A: density, volume and weight B: solid
... 9-How many grams of silver chloride are produced from 5.0g of silver nitrate reacting with an excess of barium chloride? 2AgNO3 + BaCl2 --> Ba(NO3)2 + 2AgCl A: 8.42 g B: 71.6 g C: 4.21 g 10-How many grams of potassium chloride are produced if 25g of potassium chlorate decompose? 2KClO3 --> 2KCl + 3O ...
... 9-How many grams of silver chloride are produced from 5.0g of silver nitrate reacting with an excess of barium chloride? 2AgNO3 + BaCl2 --> Ba(NO3)2 + 2AgCl A: 8.42 g B: 71.6 g C: 4.21 g 10-How many grams of potassium chloride are produced if 25g of potassium chlorate decompose? 2KClO3 --> 2KCl + 3O ...
AP CHEMISTRY MRS. SPENCER CHAPTER 4 TEST: SOLUTION
... included below only 1 of the 3 reactions listed in this question.) 4. For (each of) the following (three) reaction(s), in part (i) write a balanced equation for the reaction and in part (ii) answer the question about the reaction. In part (i), coefficients should be in terms of lowest whole numbers. ...
... included below only 1 of the 3 reactions listed in this question.) 4. For (each of) the following (three) reaction(s), in part (i) write a balanced equation for the reaction and in part (ii) answer the question about the reaction. In part (i), coefficients should be in terms of lowest whole numbers. ...
Recaps and Additional Slides Chem 20B: Reference
... Recap of Lecture #6: Thermodynamics I ΔG = ΔH – TΔS So, ΔH < 0, making stronger bonds, is favorable So, ΔS > 0, increased disorder, is favorable ΔH and ΔS vary little with temperature. ΔG does vary with T è effect of ΔS ΔG < 0 Keq > 1 Spontaneous ΔG > 0 Keq < 1 Not spontaneous ΔG = 0 Keq = 1 System ...
... Recap of Lecture #6: Thermodynamics I ΔG = ΔH – TΔS So, ΔH < 0, making stronger bonds, is favorable So, ΔS > 0, increased disorder, is favorable ΔH and ΔS vary little with temperature. ΔG does vary with T è effect of ΔS ΔG < 0 Keq > 1 Spontaneous ΔG > 0 Keq < 1 Not spontaneous ΔG = 0 Keq = 1 System ...
stoichiometry
... 23) How many grams of copper are required to replace 4.00 g of silver nitrate which is dissolved in water? ...
... 23) How many grams of copper are required to replace 4.00 g of silver nitrate which is dissolved in water? ...
AP Ch 3 Stoichiometry
... 3. Divide each by the smallest number of moles to obtain the simplest whole number ratio. 4. If whole numbers are not obtained* in step 3), multiply through by the smallest number that will give all whole numbers ...
... 3. Divide each by the smallest number of moles to obtain the simplest whole number ratio. 4. If whole numbers are not obtained* in step 3), multiply through by the smallest number that will give all whole numbers ...
Calculations with Chemical Formulas and Equations Chapter 3
... Relations in Chemical Reactions Stoichiometry is the calculation of the quantities of reactants and products involved in a chemical reaction. It is based on the balanced chemical equation and on the relationship between mass and moles. Such calculations are fundamental to most quantitative work in c ...
... Relations in Chemical Reactions Stoichiometry is the calculation of the quantities of reactants and products involved in a chemical reaction. It is based on the balanced chemical equation and on the relationship between mass and moles. Such calculations are fundamental to most quantitative work in c ...
1999 Free-Response Questions
... Directions: NO CALCULATORS MAY BE USED WITH PART B. Answer EITHER Question 7 OR Question 8. Only one of these two questions will be graded. If you start both questions, be sure to cross out the question you do not want graded. The Section II score weighting for the question you choose is 15 percent. ...
... Directions: NO CALCULATORS MAY BE USED WITH PART B. Answer EITHER Question 7 OR Question 8. Only one of these two questions will be graded. If you start both questions, be sure to cross out the question you do not want graded. The Section II score weighting for the question you choose is 15 percent. ...
Chemical Quantities(mole).
... 2. Mole to mole (ratio) 3. Mole to mass c. Limiting Reagent (or reactant): The reagent that limits or determines the amount of substance (product) that is formed in a reaction. Excess reagent (reactant): any substance (reactant) that is left over. ...
... 2. Mole to mole (ratio) 3. Mole to mass c. Limiting Reagent (or reactant): The reagent that limits or determines the amount of substance (product) that is formed in a reaction. Excess reagent (reactant): any substance (reactant) that is left over. ...
CHAPTER 9 Notes
... c. When 2.50 g of K and 1.00 g Cl2 react together, the mass of KCl produced is _____2.10 g_______________, the limiting reactant is____Cl2____________, and the reactant in excess is _______K__________________. ...
... c. When 2.50 g of K and 1.00 g Cl2 react together, the mass of KCl produced is _____2.10 g_______________, the limiting reactant is____Cl2____________, and the reactant in excess is _______K__________________. ...
2 - mrstorie
... 6. At 773 K, the reaction 2 NO (g) + O2 (g) 2 NO2 (g) produces the following concentrations: [NO] = 3.49 X 10-4M; [O2] = 0.80M; [NO2] = 0.25M. a. What is the equilibrium constant expression for this reaction? Kc = [NO]2/[NO]2[O2] b. What is the equilibrium constant for the reaction? 6.4 x 105 7. ...
... 6. At 773 K, the reaction 2 NO (g) + O2 (g) 2 NO2 (g) produces the following concentrations: [NO] = 3.49 X 10-4M; [O2] = 0.80M; [NO2] = 0.25M. a. What is the equilibrium constant expression for this reaction? Kc = [NO]2/[NO]2[O2] b. What is the equilibrium constant for the reaction? 6.4 x 105 7. ...
Unit 14-Chemical Reactions
... • Take one element at a time, working left to right except for H and O. Save H for next to last, and O until last. • IF everything balances except for O, and there is no way to balance O with a whole number, double all the coefficients and try again. (Because O is diatomic as ...
... • Take one element at a time, working left to right except for H and O. Save H for next to last, and O until last. • IF everything balances except for O, and there is no way to balance O with a whole number, double all the coefficients and try again. (Because O is diatomic as ...
g moles molarity
... occurs when solutions of Cu(NO3)2 and NaOH are mixed. What volume of 0.106 M Cu(NO3)2 solution is required to form 6.52 g of solid Cu(OH)2? 1. Check for charge dense ions that can precipitate 2. Write a net ionic reaction which excludes spectators (low charge dense ions) 3. Count total moles of all ...
... occurs when solutions of Cu(NO3)2 and NaOH are mixed. What volume of 0.106 M Cu(NO3)2 solution is required to form 6.52 g of solid Cu(OH)2? 1. Check for charge dense ions that can precipitate 2. Write a net ionic reaction which excludes spectators (low charge dense ions) 3. Count total moles of all ...
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.