unit 6 - writing and balancing chemical equations
... the total mass of the products of the change is, within measurable limits, the same as the total mass of the reactants. The formulation of this law near the end of the eighteenth century marked the beginning of modern chemistry. By that time many elements had been isolated and identified, most notab ...
... the total mass of the products of the change is, within measurable limits, the same as the total mass of the reactants. The formulation of this law near the end of the eighteenth century marked the beginning of modern chemistry. By that time many elements had been isolated and identified, most notab ...
NC PowerPoints - Taylor High School
... pentyl ethanoate is used in nail varnish for example. Ethyl ethanoate is one of a number of solvents used to extract caffeine from coffee and tea. De-caffeinated products produced with ethyl ethanoate are often described on the packaging as "naturally decaffeinated" because ethyl ethanoate is a chem ...
... pentyl ethanoate is used in nail varnish for example. Ethyl ethanoate is one of a number of solvents used to extract caffeine from coffee and tea. De-caffeinated products produced with ethyl ethanoate are often described on the packaging as "naturally decaffeinated" because ethyl ethanoate is a chem ...
Multiple Choice Questions
... Ans: Ethanol can form hydrogen bonds with water molecules, but ethane cannot. When ethanol dissolves, the decrease in the system's entropy that results from formation of ordered arrays of water around the CH3CH2– group is partly compensated by the favorable interactions (hydrogen bonds) of the hydro ...
... Ans: Ethanol can form hydrogen bonds with water molecules, but ethane cannot. When ethanol dissolves, the decrease in the system's entropy that results from formation of ordered arrays of water around the CH3CH2– group is partly compensated by the favorable interactions (hydrogen bonds) of the hydro ...
Pb2+ +2I- → PbI2 (s)
... What is the difference between a Bronsted-Lowry acid/base reaction and a Lewis acid/base reaction? Bronsted lowry acids give H+, Lewis bases give an electron ...
... What is the difference between a Bronsted-Lowry acid/base reaction and a Lewis acid/base reaction? Bronsted lowry acids give H+, Lewis bases give an electron ...
Chapter 4 Aqueous Reactions and Solution Stoichiometry
... • HCl, HBr, HI, HNO3, HClO3, HClO4 and H2SO4 are all strong acids. All other acids are assumed to be weak acids. • A weak acid or weak base only partially ionizes (dissociates) in aqueous solution. • Amphiprotic substances can behave as either a proton acceptor or a proton donor. Water is an example ...
... • HCl, HBr, HI, HNO3, HClO3, HClO4 and H2SO4 are all strong acids. All other acids are assumed to be weak acids. • A weak acid or weak base only partially ionizes (dissociates) in aqueous solution. • Amphiprotic substances can behave as either a proton acceptor or a proton donor. Water is an example ...
Chemistry 12 is an intensive course, covering a great deal of
... Assignments will be given daily. Students are responsible for catching up and completing any missed assignments due to absences as soon as possible. Missed tests must be made up the next class present (within a one week period) or be given a mark of zero or omitted at the discretion of the teacher. ...
... Assignments will be given daily. Students are responsible for catching up and completing any missed assignments due to absences as soon as possible. Missed tests must be made up the next class present (within a one week period) or be given a mark of zero or omitted at the discretion of the teacher. ...
Advanced Chemical Reactions
... pressure increase favors the reaction that produces fewer molecules (stoichiometry) 2NOCl 2 NO + Cl2 H2O + CO H2 + CO2 ...
... pressure increase favors the reaction that produces fewer molecules (stoichiometry) 2NOCl 2 NO + Cl2 H2O + CO H2 + CO2 ...
PART 2 – CHEMISTRY
... neutrons. Around this, electrons orbit at high speed. The atomic number is the number of protons in the nucleus. The mass number is the total number of protons and neutrons in the nucleus. For example, the atomic number of fluorine is 9. This means that there are 9 protons in the nucleus and 9 elec ...
... neutrons. Around this, electrons orbit at high speed. The atomic number is the number of protons in the nucleus. The mass number is the total number of protons and neutrons in the nucleus. For example, the atomic number of fluorine is 9. This means that there are 9 protons in the nucleus and 9 elec ...
FREE Sample Here
... Ans: Ethanol can form hydrogen bonds with water molecules, but ethane cannot. When ethanol dissolves, the decrease in the system's entropy that results from formation of ordered arrays of water around the CH3CH2– group is partly compensated by the favorable interactions (hydrogen bonds) of the hydro ...
... Ans: Ethanol can form hydrogen bonds with water molecules, but ethane cannot. When ethanol dissolves, the decrease in the system's entropy that results from formation of ordered arrays of water around the CH3CH2– group is partly compensated by the favorable interactions (hydrogen bonds) of the hydro ...
File
... precipitate forms. Once the reaction is complete, which ion is present IN THE SOLUTION in lowest concentration? A) Ca2+ B) Na+ C) NO3– D) PO4321. What is the % NITROGEN by mass in the compound Al(NO3)3? A) 6.57% B) 19.7 % C) 15.7 % D) 46.1 % 22. Oxalic acid is 2.22 % hydrogen, 26.67% carbon, and 71. ...
... precipitate forms. Once the reaction is complete, which ion is present IN THE SOLUTION in lowest concentration? A) Ca2+ B) Na+ C) NO3– D) PO4321. What is the % NITROGEN by mass in the compound Al(NO3)3? A) 6.57% B) 19.7 % C) 15.7 % D) 46.1 % 22. Oxalic acid is 2.22 % hydrogen, 26.67% carbon, and 71. ...
Atoms, Molecules and Ions
... (b) There are two silicon atoms and six bromine atoms present, so the formula is Si2Br6. ...
... (b) There are two silicon atoms and six bromine atoms present, so the formula is Si2Br6. ...
Fall.2008.Week9.Lesson.2 - reich
... two things does fire require? O2 and something to burn. We normally burn hydrocarbons (Hydro=H, Carbon = C therefore stuff made up of H and C). • The products are always CO2 and H2O. • Methane and Oxygen burn write the equation. • ___CH4+ ___O2 ___ CO2 + ___H2O ...
... two things does fire require? O2 and something to burn. We normally burn hydrocarbons (Hydro=H, Carbon = C therefore stuff made up of H and C). • The products are always CO2 and H2O. • Methane and Oxygen burn write the equation. • ___CH4+ ___O2 ___ CO2 + ___H2O ...
Name AP Chemistry Take Home Quiz – Due Thursday, 1/9/2014
... a. CN-(aq) is a stronger base than C2H3O2-(aq) b. HCN(aq) is a stronger acid than HC2H3O2(aq) c. The conjugate base of CN-(aq) is C2H3O2-(aq) d. The equilibrium constant will increase with an increase in temperature. e. The pH of a solution containing equimolar amounts of CN-(aq) and HC2H3O2(aq) is ...
... a. CN-(aq) is a stronger base than C2H3O2-(aq) b. HCN(aq) is a stronger acid than HC2H3O2(aq) c. The conjugate base of CN-(aq) is C2H3O2-(aq) d. The equilibrium constant will increase with an increase in temperature. e. The pH of a solution containing equimolar amounts of CN-(aq) and HC2H3O2(aq) is ...
Chem 1711 Review Exam 2
... major areas we have discussed. You are responsible for all material covered in lecture and in the text. Chapter 4: Chemical Reactions The Nature of Solutions: • speciation and stoichiometry associated with the dissolution of ionic vs. molecular compounds in water • strong vs. weak vs. nonelectrolyte ...
... major areas we have discussed. You are responsible for all material covered in lecture and in the text. Chapter 4: Chemical Reactions The Nature of Solutions: • speciation and stoichiometry associated with the dissolution of ionic vs. molecular compounds in water • strong vs. weak vs. nonelectrolyte ...
1) In the reaction H2O + CH3COOH H3O+ + CH3COO
... 8) (20 points) For the elementary reaction series A+B C D, for components C and D only, give a) the rate equations (differential equations describing the rate of change in concentration of each component with time), b) the values of the initial rates of change of C and D and c) the final conce ...
... 8) (20 points) For the elementary reaction series A+B C D, for components C and D only, give a) the rate equations (differential equations describing the rate of change in concentration of each component with time), b) the values of the initial rates of change of C and D and c) the final conce ...
Solution
... ClO radicals in the stratosphere are formed from the reaction of Cl atoms with O3. The Cl atoms in turn are generated when sunlight hits CFCs like CF2Cl2 (also known as Freon-12). Calculate the maximum wavelength (in nanometers) required to break a C-Cl bond in CF2Cl2 using the data on Page 2. C-Cl ...
... ClO radicals in the stratosphere are formed from the reaction of Cl atoms with O3. The Cl atoms in turn are generated when sunlight hits CFCs like CF2Cl2 (also known as Freon-12). Calculate the maximum wavelength (in nanometers) required to break a C-Cl bond in CF2Cl2 using the data on Page 2. C-Cl ...
Density functional theory and FTIR spectroscopic study of carboxyl
... Received 29 March 2005;revised 7 September 2005;accepted 30 September 2005 Both molecular modelling and FTIR have been used to study carboxyl group among acetic acid, potassium and sodium acetate, glycine, sodium salicylate, salicylic acid and cellulose acetate. Molecular modelling was used to study ...
... Received 29 March 2005;revised 7 September 2005;accepted 30 September 2005 Both molecular modelling and FTIR have been used to study carboxyl group among acetic acid, potassium and sodium acetate, glycine, sodium salicylate, salicylic acid and cellulose acetate. Molecular modelling was used to study ...
FREE Sample Here
... E) The strength of a hydrogen bond depends on the linearity of the three atoms involved in the bond. 2. Weak interactions in aqueous systems Page: 48 Difficulty: 2 Ans: A A true statement about hydrophobic interactions is that they: ...
... E) The strength of a hydrogen bond depends on the linearity of the three atoms involved in the bond. 2. Weak interactions in aqueous systems Page: 48 Difficulty: 2 Ans: A A true statement about hydrophobic interactions is that they: ...
Acid
An acid (from the Latin acidus/acēre meaning sour) is a chemical substance whose aqueous solutions are characterized by a sour taste, the ability to turn blue litmus red, and the ability to react with bases and certain metals (like calcium) to form salts. Aqueous solutions of acids have a pH of less than 7. Non-aqueous acids are usually formed when an anion (negative ion) reacts with one or more positively charged hydrogen cations. A lower pH means a higher acidity, and thus a higher concentration of positive hydrogen ions in the solution. Chemicals or substances having the property of an acid are said to be acidic.There are three common definitions for acids: the Arrhenius definition, the Brønsted-Lowry definition, and the Lewis definition. The Arrhenius definition defines acids as substances which increase the concentration of hydrogen ions (H+), or more accurately, hydronium ions (H3O+), when dissolved in water. The Brønsted-Lowry definition is an expansion: an acid is a substance which can act as a proton donor. By this definition, any compound which can easily be deprotonated can be considered an acid. Examples include alcohols and amines which contain O-H or N-H fragments. A Lewis acid is a substance that can accept a pair of electrons to form a covalent bond. Examples of Lewis acids include all metal cations, and electron-deficient molecules such as boron trifluoride and aluminium trichloride.Common examples of acids include hydrochloric acid (a solution of hydrogen chloride which is found in gastric acid in the stomach and activates digestive enzymes), acetic acid (vinegar is a dilute solution of this liquid), sulfuric acid (used in car batteries), and tartaric acid (a solid used in baking). As these examples show, acids can be solutions or pure substances, and can be derived from solids, liquids, or gases. Strong acids and some concentrated weak acids are corrosive, but there are exceptions such as carboranes and boric acid.