AP Chemistry Summer Assignment THIS
... you recover? Is this enough copper to react with all 6 moles of silver ions? ...
... you recover? Is this enough copper to react with all 6 moles of silver ions? ...
how reactions occur
... without being used up in the reaction. • Homogeneous catalysts are substances that are distributed uniformly throughout a reaction mixture. • Heterogeneous catalysts are substances normally used in the form of solids with large surface areas on which the reactions take place. • One explanation for c ...
... without being used up in the reaction. • Homogeneous catalysts are substances that are distributed uniformly throughout a reaction mixture. • Heterogeneous catalysts are substances normally used in the form of solids with large surface areas on which the reactions take place. • One explanation for c ...
Dear Chemistry Student, I am excited that you have chosen to
... 20. HCl + NaOH → NaCl + H2O a. Given that there is 2 moles of HCl and 2.5 moles of NaOH reacting, find the limiting reactant (hint: write a balanced equation). 21. 2HNO3(aq) + 3H2S(g) -> 2NO(g) + 4H2O(l) +3S(s) In the reaction above, 4.62g HNO3(aq) and 1.84g H2S(g) are mixed. How many grams of NO(g) ...
... 20. HCl + NaOH → NaCl + H2O a. Given that there is 2 moles of HCl and 2.5 moles of NaOH reacting, find the limiting reactant (hint: write a balanced equation). 21. 2HNO3(aq) + 3H2S(g) -> 2NO(g) + 4H2O(l) +3S(s) In the reaction above, 4.62g HNO3(aq) and 1.84g H2S(g) are mixed. How many grams of NO(g) ...
de Caux - Combustion of Methane Demonstration
... o Perform activities to investigate exothermic and endothermic chemical reactions. o Show concern for safety and accept the need for rules and regulations. CR3 Identify characteristics of chemical reactions involving organic compounds o Observe and describe the combustion process. o Illustrate, us ...
... o Perform activities to investigate exothermic and endothermic chemical reactions. o Show concern for safety and accept the need for rules and regulations. CR3 Identify characteristics of chemical reactions involving organic compounds o Observe and describe the combustion process. o Illustrate, us ...
Practice Test 1 (Chapters 1-7)
... 23. Which of the following is a chemical change? a. Water condenses on a mirror. b. A damp towel dries. c. Peanuts are crushed. d. A “tin” can rusts. e. At least two of the above (a-d) exhibit a ...
... 23. Which of the following is a chemical change? a. Water condenses on a mirror. b. A damp towel dries. c. Peanuts are crushed. d. A “tin” can rusts. e. At least two of the above (a-d) exhibit a ...
Atom (A) or Ion
... 61. What unit for temperature is used for all gas law problems? 62. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? 63. Define “mole ...
... 61. What unit for temperature is used for all gas law problems? 62. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? 63. Define “mole ...
Atom (A) or Ion (I)
... 61. What unit for temperature is used for all gas law problems? 62. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? 63. Define “mole ...
... 61. What unit for temperature is used for all gas law problems? 62. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? 63. Define “mole ...
Atom (A) or Ion (I)
... 61. What unit for temperature is used for all gas law problems? 62. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? 63. Define “mole ...
... 61. What unit for temperature is used for all gas law problems? 62. If I initially have a gas at a pressure of 12 atm, a volume of 23 liters, and a temperature of 200 K, and then I raise the pressure to 14 atm and increase the temperature to 300 K, what is the new volume of the gas? 63. Define “mole ...
How many grams of oxygen are made if 3.75 moles of KClO 3
... 11. The characteristic odor of garlic is due to allyl sulfide (C3H5)2S. A recipe for hummus calls for garlic that contains no more than 6.89 mol of allyl sulfide. You were hired by Cedar as a chemistry consultant to calculate the maximum mass of allyl sulfide that should be included in the recipe fo ...
... 11. The characteristic odor of garlic is due to allyl sulfide (C3H5)2S. A recipe for hummus calls for garlic that contains no more than 6.89 mol of allyl sulfide. You were hired by Cedar as a chemistry consultant to calculate the maximum mass of allyl sulfide that should be included in the recipe fo ...
Chapter 12
... By international agreement, an atom of the carbon isotope (called carbon-12) that has 6 protons and 6 neutrons has a mass of exactly 12 atomic mass units (amu). This carbon-12 atom serves as the standard, so one atomic mass unit is defined as amass exactly equal to one-twelfth the mass of one carbon ...
... By international agreement, an atom of the carbon isotope (called carbon-12) that has 6 protons and 6 neutrons has a mass of exactly 12 atomic mass units (amu). This carbon-12 atom serves as the standard, so one atomic mass unit is defined as amass exactly equal to one-twelfth the mass of one carbon ...
Determination of the Molar Volume of H2(g) and of O2(g)
... these gases by downward displacement of water. This technique will be demonstrated by the teacher. A. Preparation of hydrogen gas, H2(g) You will produce hydrogen gas according to the unbalanced chemical equation: 1 Mg(s) + ____HCl(aq) Æ ____MgCl2(aq) + ____H2(g) ...
... these gases by downward displacement of water. This technique will be demonstrated by the teacher. A. Preparation of hydrogen gas, H2(g) You will produce hydrogen gas according to the unbalanced chemical equation: 1 Mg(s) + ____HCl(aq) Æ ____MgCl2(aq) + ____H2(g) ...
How to Balance Chemical Equations
... inventory on that side of the chemical equation. Repeat the process until total number of atoms for each element perfectly matches on both sides of the chemical equation. ...
... inventory on that side of the chemical equation. Repeat the process until total number of atoms for each element perfectly matches on both sides of the chemical equation. ...
Chapter 3 PowerPoint
... Commercial brass is an alloy of Cu and Zn. It reacts with HCl by the following reaction Zn(s) + 2HCl(aq) ZnCl2 (aq) + H2(g) Cu does not react. When 0.5065 g of brass is reacted with excess HCl, 0.0985 g of ZnCl2 are eventually isolated. What is the composition of the brass? ...
... Commercial brass is an alloy of Cu and Zn. It reacts with HCl by the following reaction Zn(s) + 2HCl(aq) ZnCl2 (aq) + H2(g) Cu does not react. When 0.5065 g of brass is reacted with excess HCl, 0.0985 g of ZnCl2 are eventually isolated. What is the composition of the brass? ...
The Basics - I`m a faculty member, and I need web space. What
... and remove an electron from a gaseous atom • 1st ionization energy: the energy required to remove the first electron • 2nd ionization energy: the energy required to remove the second electron • 3rd ionization energy: the energy required removing the third electron • Trend: ionization energy increase ...
... and remove an electron from a gaseous atom • 1st ionization energy: the energy required to remove the first electron • 2nd ionization energy: the energy required to remove the second electron • 3rd ionization energy: the energy required removing the third electron • Trend: ionization energy increase ...
Stoichiometry: Calculations with Chemical Formulas and Equations
... • In a lab, we cannot work with individual molecules. They are too small. • 6.02 × 1023 atoms or molecules is an amount that brings us to lab size. It is ONE MOLE. • One mole of 12C has a mass of 12.000 g. © 2015 Pearson Education, Inc. ...
... • In a lab, we cannot work with individual molecules. They are too small. • 6.02 × 1023 atoms or molecules is an amount that brings us to lab size. It is ONE MOLE. • One mole of 12C has a mass of 12.000 g. © 2015 Pearson Education, Inc. ...
Study Guide for Test 2: Chapters 3 & 4... This is NOT a complete list of what will be... Revised March 4, 2014
... 11) Still know Avogadro’s Number (Chapter 2) and be able to convert between number of items (atoms, molecules, ions, etc.) and moles of that item. Be able to combine this calculation with molar mass. (1 mole items = 6.022 x 1023 items) 12) Be able to convert between moles of a compound and moles of ...
... 11) Still know Avogadro’s Number (Chapter 2) and be able to convert between number of items (atoms, molecules, ions, etc.) and moles of that item. Be able to combine this calculation with molar mass. (1 mole items = 6.022 x 1023 items) 12) Be able to convert between moles of a compound and moles of ...
Chemical Equation Interpretations – Match the chemical equation
... D. When octane and oxygen gas are burned in our cards, carbon dioxide and water come out in the exhaust. E. Methanol , if ingested, reacts with oxygen to form formaldehyde, which is toxic. Water is also formed in this reaction. F. Liquid mercury evaporates to produce mercury vapor. G. Saturated fatt ...
... D. When octane and oxygen gas are burned in our cards, carbon dioxide and water come out in the exhaust. E. Methanol , if ingested, reacts with oxygen to form formaldehyde, which is toxic. Water is also formed in this reaction. F. Liquid mercury evaporates to produce mercury vapor. G. Saturated fatt ...
Entropy and reaction spontaneity Gibbs free energy
... If, in the reaction mixture of a reaction at equilibrium, one increases activities (concentrations, pressures) of the reactants, the reaction will move to the right (toward products), reducing the denominator and increasing the numerator to maintain the constancy of K; If one increases activitie ...
... If, in the reaction mixture of a reaction at equilibrium, one increases activities (concentrations, pressures) of the reactants, the reaction will move to the right (toward products), reducing the denominator and increasing the numerator to maintain the constancy of K; If one increases activitie ...
Physical and Chemical change: Introduction
... 2. Take some of this mixture and place it in the test tube. The test tube should be about 1/3 full. 3. This reaction should ideally take place in a fume cupboard. Heat the test tube containing the mixture over the Bunsen burner. Increase the heat if no reaction takes place. Once the reaction begins, ...
... 2. Take some of this mixture and place it in the test tube. The test tube should be about 1/3 full. 3. This reaction should ideally take place in a fume cupboard. Heat the test tube containing the mixture over the Bunsen burner. Increase the heat if no reaction takes place. Once the reaction begins, ...
SCH3U Course Review
... decrease across a period from left to right increase across a period from left to right increase as you go down a family ...
... decrease across a period from left to right increase across a period from left to right increase as you go down a family ...
Molar Heat of Reaction
... Dissolve 6.69 g of lithium chloride (LiCl) in 100 mL of water at 24.2°C in a calorimeter. The final temperature of the water is 37.4°C a) What is the molar heat of dissolution (ΔHd) of lithium chloride b) Write the thermochemical equation for the dissolution of LiCl, incorporating the calculated val ...
... Dissolve 6.69 g of lithium chloride (LiCl) in 100 mL of water at 24.2°C in a calorimeter. The final temperature of the water is 37.4°C a) What is the molar heat of dissolution (ΔHd) of lithium chloride b) Write the thermochemical equation for the dissolution of LiCl, incorporating the calculated val ...
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.