New AQA C3 revison guide
... The carbon reduces the levels of chlorine, pesticides and other organic impurities in the water. The ion-exchange column removes calcium, magnesium, lead, copper and aluminium ions. The silver discourages the growth of bacteria in the cartridge. In most jugs the cartridge needs to be changed eve ...
... The carbon reduces the levels of chlorine, pesticides and other organic impurities in the water. The ion-exchange column removes calcium, magnesium, lead, copper and aluminium ions. The silver discourages the growth of bacteria in the cartridge. In most jugs the cartridge needs to be changed eve ...
practice unit #2 exam
... D. the powdered form has more surface area. 7. The series of steps that most reactions undergo, from initial reactants to final products, is called the: A. catalytic conversion ...
... D. the powdered form has more surface area. 7. The series of steps that most reactions undergo, from initial reactants to final products, is called the: A. catalytic conversion ...
Chem 206 Exam 2 Answers
... Or: Because at equilibrium kf=kr, 3.45 M −1 ⋅ s −1 × 2.8 × 2.8 = 27 M ⋅ s−1 d) After equilibrium is obtained, you add a catalyst and 3.00 additional moles of HCl. What will happen? <8 pts.> The addition of a catalyst will not change the equilibrium but will only increase the rate at which equilibriu ...
... Or: Because at equilibrium kf=kr, 3.45 M −1 ⋅ s −1 × 2.8 × 2.8 = 27 M ⋅ s−1 d) After equilibrium is obtained, you add a catalyst and 3.00 additional moles of HCl. What will happen? <8 pts.> The addition of a catalyst will not change the equilibrium but will only increase the rate at which equilibriu ...
Unit 3 Revision Notes 213.00KB 2017-03-01 18
... 3) No lime scale is formed. There are 2 popular methods 1) Calcium ions may be taken out of solution by adding another ion to form an insoluble calcium salt. e.g. Sodium carbonate (washing soda) reacts to form insoluble calcium carbonate. 2) An ion exchange resin can be used. This is a material cont ...
... 3) No lime scale is formed. There are 2 popular methods 1) Calcium ions may be taken out of solution by adding another ion to form an insoluble calcium salt. e.g. Sodium carbonate (washing soda) reacts to form insoluble calcium carbonate. 2) An ion exchange resin can be used. This is a material cont ...
1996 Free Response Answers
... The cell potential would increase Since all ions are at 1 M, Q for the system is 1 and E° = (RT/nF) ln K so as T increases, so should E° Note: no credit lost if student recognizes Keq dependence on T. For temperature change in this problem, decrease in ln K term is small relative to the term RT/nF ...
... The cell potential would increase Since all ions are at 1 M, Q for the system is 1 and E° = (RT/nF) ln K so as T increases, so should E° Note: no credit lost if student recognizes Keq dependence on T. For temperature change in this problem, decrease in ln K term is small relative to the term RT/nF ...
Summer_Assignment_AP_Chemistry_TW 2015
... To the AP Chemistry Student: Welcome to my AP Chemistry class! I am looking forward to helping you gain a deeper appreciation for the science of chemistry and how it impacts our lives. I hope you are looking forward to an exciting and challenging year. Since you have elected to take this course, I a ...
... To the AP Chemistry Student: Welcome to my AP Chemistry class! I am looking forward to helping you gain a deeper appreciation for the science of chemistry and how it impacts our lives. I hope you are looking forward to an exciting and challenging year. Since you have elected to take this course, I a ...
Chemistry 520 - Problem Set 6
... Calculate the temperature of the atmosphere 10 km above the earth where = 210 Torr. The temperature and pressure at the surface of the earth (0 km) are 25C and 760 Torr, respectively. You may assume air behaves as an ideal gas with P = 72 . You may ignore gravitational in uences. [-66.6C] To solve ...
... Calculate the temperature of the atmosphere 10 km above the earth where = 210 Torr. The temperature and pressure at the surface of the earth (0 km) are 25C and 760 Torr, respectively. You may assume air behaves as an ideal gas with P = 72 . You may ignore gravitational in uences. [-66.6C] To solve ...
Inorganic and organic chemistry 2
... the final titre. Check that you would get 7 (or 6.96 which is what is obtained using the 19.6 g). It is only the last couple of steps in the calculation that are different. Check it out below. Moles of MnO4− = ...
... the final titre. Check that you would get 7 (or 6.96 which is what is obtained using the 19.6 g). It is only the last couple of steps in the calculation that are different. Check it out below. Moles of MnO4− = ...
Cool Chemical Reactions Lab Partners: Background Information
... Zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas. Zn + 2 HCl ZnCl2 + H2 The “Hear It Pop” experiment was a single replacement reaction because the reaction started with one compound and one element and the products were also one compound and one element. It followed the pa ...
... Zinc reacts with hydrochloric acid to form zinc chloride and hydrogen gas. Zn + 2 HCl ZnCl2 + H2 The “Hear It Pop” experiment was a single replacement reaction because the reaction started with one compound and one element and the products were also one compound and one element. It followed the pa ...
1. Write the balanced equation for the combustion of butane (C4H10
... 1. Write the balanced equation for the combustion of butane (C4H10 ). Then, show what the following molar ratios should be. a. C4H10 / O2 b. O2 / CO2 c. O2 / H2O d. C4H10 / CO2 e. C4H10 / H2O 2. How many moles of O2 can be produced by the decomposition of 12.00 moles of KClO3? 3. Potassium chloride ...
... 1. Write the balanced equation for the combustion of butane (C4H10 ). Then, show what the following molar ratios should be. a. C4H10 / O2 b. O2 / CO2 c. O2 / H2O d. C4H10 / CO2 e. C4H10 / H2O 2. How many moles of O2 can be produced by the decomposition of 12.00 moles of KClO3? 3. Potassium chloride ...
Answers to NHSCE 2002 Part A Page 1
... have the same molecular formulae but different structural formulae or connectivity. These isomers are called constitutional isomers (their former name was structural isomers). The molecular formula of (CH3)2O is C2H6O, and the alcohol with this molecular formula is C2H5OH. (The formula CH3-O-CH3 i ...
... have the same molecular formulae but different structural formulae or connectivity. These isomers are called constitutional isomers (their former name was structural isomers). The molecular formula of (CH3)2O is C2H6O, and the alcohol with this molecular formula is C2H5OH. (The formula CH3-O-CH3 i ...
File
... V. A compound is 41.07 % K, 33.72 % S, and also contains oxygen. Find the empirical formula for the compound. ( 3 pts) VI. Find the molecular formula of a hydrocarbon which is 80.0 % carbon by mass and has a molecular mass of 30.0. ( 3 pts) VII. When alcohols are burned in excess oxygen, they produc ...
... V. A compound is 41.07 % K, 33.72 % S, and also contains oxygen. Find the empirical formula for the compound. ( 3 pts) VI. Find the molecular formula of a hydrocarbon which is 80.0 % carbon by mass and has a molecular mass of 30.0. ( 3 pts) VII. When alcohols are burned in excess oxygen, they produc ...
Chapter 6: Chemical Equilibrium
... 9. The reaction, Q + 2 SO3(g) 2 SO2(g) + O2(g) is endothermic. Predict what will happen if the temperature is increased. a. Kc remains the same b. Kc decreases c. the pressure decreases d. more SO3(g) is produced * e. Kc increases T increase, reaction will shift to right side and Kc increase 10. Con ...
... 9. The reaction, Q + 2 SO3(g) 2 SO2(g) + O2(g) is endothermic. Predict what will happen if the temperature is increased. a. Kc remains the same b. Kc decreases c. the pressure decreases d. more SO3(g) is produced * e. Kc increases T increase, reaction will shift to right side and Kc increase 10. Con ...
The Periodic Table HL Page 1 of 3 G. Galvin Name: Periodic Table
... -derive the electronic configurations of ions of s- and p-block elements only -describe the arrangement of electrons in individual orbitals of p-block atoms ...
... -derive the electronic configurations of ions of s- and p-block elements only -describe the arrangement of electrons in individual orbitals of p-block atoms ...
KINETICS AND EQUILIBRIUM
... chemical reaction should not be confused with the sign for H. a. The sign of H tells us whether a reaction is endothermic or exothermic. b. If H is positive the energy term is found on the reactant side the reaction is endothermic. c. conversely if H is negative the energy term is found on the p ...
... chemical reaction should not be confused with the sign for H. a. The sign of H tells us whether a reaction is endothermic or exothermic. b. If H is positive the energy term is found on the reactant side the reaction is endothermic. c. conversely if H is negative the energy term is found on the p ...
01 - Cobb Learning
... Match the correct description with the correct term. Write the letter in the space provided. ...
... Match the correct description with the correct term. Write the letter in the space provided. ...
PCSD General Chemistry Pacing Guide
... Explain the history and models of the atomic theory through Democritus, Dalton, Thomson, Rutherford, Chadwick, Bohr, and the electron cloud model Describe how Dalton’s atomic theory has changed over time Identify the parts of the atom Define atomic number, mass number, and atomic mass and use these ...
... Explain the history and models of the atomic theory through Democritus, Dalton, Thomson, Rutherford, Chadwick, Bohr, and the electron cloud model Describe how Dalton’s atomic theory has changed over time Identify the parts of the atom Define atomic number, mass number, and atomic mass and use these ...
Unit 6 Chemical Equations and Reactions Balancing Equations
... 6. Aluminum metal is oxidized by oxygen (from the air) to form aluminum oxide. 4 Al (s) + 3 O2 → 2 Al2O3 7. Sodium oxide reacts with carbon dioxide to form sodium carbonate. Na2O + CO2 → Na2 CO3 8. Calcium metal reacts with water to form calcium hydroxide and hydrogen gas. Ca (s) + 2H2O → Ca(OH)2 + ...
... 6. Aluminum metal is oxidized by oxygen (from the air) to form aluminum oxide. 4 Al (s) + 3 O2 → 2 Al2O3 7. Sodium oxide reacts with carbon dioxide to form sodium carbonate. Na2O + CO2 → Na2 CO3 8. Calcium metal reacts with water to form calcium hydroxide and hydrogen gas. Ca (s) + 2H2O → Ca(OH)2 + ...
Unit 2 - Calderglen High School
... (c) Aldehydes can also be formed by the reaction of some alcohols with copper(II) oxide. Name the type of alcohol that would react with copper(II) oxide to form an aldehyde. ...
... (c) Aldehydes can also be formed by the reaction of some alcohols with copper(II) oxide. Name the type of alcohol that would react with copper(II) oxide to form an aldehyde. ...
Chapter Five
... The substance(s) which we begin with are called the reactant(s) The substance(s) which we end with are called the product(s) We will examine chemical reactions in greater depth in Chapter Eight Writing Chemical Equations Chemical equations are written with the reactants to the left, the prod ...
... The substance(s) which we begin with are called the reactant(s) The substance(s) which we end with are called the product(s) We will examine chemical reactions in greater depth in Chapter Eight Writing Chemical Equations Chemical equations are written with the reactants to the left, the prod ...
H2 Chemistry Syllabus (9729)
... feasibility of a reaction – the Gibbs free energy (∆G). For aqueous redox reactions, the more convenient notion of electrode potential (E) is used, and the resultant cell potential (Ecell) gives a measure of thermodynamics feasibility instead. The chemical kinetics facet of a reaction can be underst ...
... feasibility of a reaction – the Gibbs free energy (∆G). For aqueous redox reactions, the more convenient notion of electrode potential (E) is used, and the resultant cell potential (Ecell) gives a measure of thermodynamics feasibility instead. The chemical kinetics facet of a reaction can be underst ...
2009 - NESACS
... For problems 12-14, use the following information: 2 KClO3(s) 2 KCl(s) + 3 O2(g) 2 KHCO3(s) K2O(s) + H2O(g) + 2 CO2(g) K2CO3(s) K2O(s) + CO2(g) Molar masses: H2O = 18.0, CO2 = 44.0, O2 = 32.0, KClO3 = 122.6, KHCO3 = 100.1, K2CO3 = 138.2, KCl = 74.55 12. A mixture of KClO3, K2CO3, KHCO3 and KCl ...
... For problems 12-14, use the following information: 2 KClO3(s) 2 KCl(s) + 3 O2(g) 2 KHCO3(s) K2O(s) + H2O(g) + 2 CO2(g) K2CO3(s) K2O(s) + CO2(g) Molar masses: H2O = 18.0, CO2 = 44.0, O2 = 32.0, KClO3 = 122.6, KHCO3 = 100.1, K2CO3 = 138.2, KCl = 74.55 12. A mixture of KClO3, K2CO3, KHCO3 and KCl ...
Redox
Redox reactions include all chemical reactions in which atoms have their oxidation state changed; in general, redox reactions involve the transfer of electrons between species. The term ""redox"" comes from two concepts involved with electron transfer: reduction and oxidation. It can be explained in simple terms: Oxidation is the loss of electrons or an increase in oxidation state by a molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion.Although oxidation reactions are commonly associated with the formation of oxides from oxygen molecules, these are only specific examples of a more general concept of reactions involving electron transfer.Redox reactions, or oxidation-reduction reactions, have a number of similarities to acid–base reactions. Like acid–base reactions, redox reactions are a matched set, that is, there cannot be an oxidation reaction without a reduction reaction happening simultaneously. The oxidation alone and the reduction alone are each called a half-reaction, because two half-reactions always occur together to form a whole reaction. When writing half-reactions, the gained or lost electrons are typically included explicitly in order that the half-reaction be balanced with respect to electric charge.Though sufficient for many purposes, these descriptions are not precisely correct. Oxidation and reduction properly refer to a change in oxidation state — the actual transfer of electrons may never occur. The oxidation state of an atom is the fictitious charge that an atom would have if all bonds between atoms of different elements were 100% ionic. Thus, oxidation is better defined as an increase in oxidation state, and reduction as a decrease in oxidation state. In practice, the transfer of electrons will always cause a change in oxidation state, but there are many reactions that are classed as ""redox"" even though no electron transfer occurs (such as those involving covalent bonds).There are simple redox processes, such as the oxidation of carbon to yield carbon dioxide (CO2) or the reduction of carbon by hydrogen to yield methane (CH4), and more complex processes such as the oxidation of glucose (C6H12O6) in the human body through a series of complex electron transfer processes.