Energetics - WordPress.com
... reactions have different values of enthalpy changes, ΔH, as different bonds with different strengths are being broken and formed. The amount (or concentration) of reactants; the greater the amount that reacts , the greater the heat change. The states of the reactants and products – changing state in ...
... reactions have different values of enthalpy changes, ΔH, as different bonds with different strengths are being broken and formed. The amount (or concentration) of reactants; the greater the amount that reacts , the greater the heat change. The states of the reactants and products – changing state in ...
acid
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
Hein and Arena - faculty at Chemeketa
... equilibrium, the system will respond in such a way as to relieve that stress and restore equilibrium under a new set of conditions. ...
... equilibrium, the system will respond in such a way as to relieve that stress and restore equilibrium under a new set of conditions. ...
CH 4 Notes
... A salt is any ionic compound whose cation comes from a base, and anion from an acid. The other product, H2O, is a common weak electrolyte. Typical examples of neutralization reactions: Reactions between an acid and a metal hydroxide. Mg(OH)2 (milk of magnesia) is a suspension As HCl is added, ...
... A salt is any ionic compound whose cation comes from a base, and anion from an acid. The other product, H2O, is a common weak electrolyte. Typical examples of neutralization reactions: Reactions between an acid and a metal hydroxide. Mg(OH)2 (milk of magnesia) is a suspension As HCl is added, ...
Types of Reactions
... Consider the reaction between Mg and HCl: Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g) • In the process the metal is oxidized and the H+1 is reduced. • Example: It is possible for metals to be oxidized in the presence of a salt: Fe (s) + Ni(NO3)2 (aq) Fe(NO3)2 (aq) + Ni (s) • The net ionic equation s ...
... Consider the reaction between Mg and HCl: Mg (s) + 2 HCl (aq) MgCl2 (aq) + H2 (g) • In the process the metal is oxidized and the H+1 is reduced. • Example: It is possible for metals to be oxidized in the presence of a salt: Fe (s) + Ni(NO3)2 (aq) Fe(NO3)2 (aq) + Ni (s) • The net ionic equation s ...
chapter4-bur.2917051..
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
AP Chemistry: Aqueous Reactions and Solution Stoichiometry
... A salt is any ionic compound whose cation comes from a base, and anion from an acid. The other product, H2O, is a common weak electrolyte. Typical examples of neutralization reactions: Reactions between an acid and a metal hydroxide. Mg(OH)2 (milk of magnesia) is a suspension As HCl is added, the ...
... A salt is any ionic compound whose cation comes from a base, and anion from an acid. The other product, H2O, is a common weak electrolyte. Typical examples of neutralization reactions: Reactions between an acid and a metal hydroxide. Mg(OH)2 (milk of magnesia) is a suspension As HCl is added, the ...
Document
... 1. Elements: The oxidation number of an atom in an element is zero. 2. Monatomic ions: The oxidation number of an atom in a monatomic ion equals the charge on the ion. 3. Oxygen: The oxidation number of oxygen is -2 in most of its compounds. (An exception is O in H2O2 and other peroxides, where the ...
... 1. Elements: The oxidation number of an atom in an element is zero. 2. Monatomic ions: The oxidation number of an atom in a monatomic ion equals the charge on the ion. 3. Oxygen: The oxidation number of oxygen is -2 in most of its compounds. (An exception is O in H2O2 and other peroxides, where the ...
MC94 - Southchemistry.com
... When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00-liter flask, the reaction represented above occurs. After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO 3. Based on these results, the eq ...
... When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00-liter flask, the reaction represented above occurs. After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO 3. Based on these results, the eq ...
Net ionic equation
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
No Slide Title
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
... because the water molecules have a partial negative charge on the oxygen atom (-) and partial positive charges on the hydrogen atoms (+), where “” indicates a small positive or negative charge. The reason these partial charges exist will be discussed later in the semester. Because cations and ani ...
chemistry 2.1
... kbookks iiss lillimited i ited imi t d to to 3% un und under der th der the he NZ NZ Copy CCopyright opy pyrig ight ht Act At Act. ...
... kbookks iiss lillimited i ited imi t d to to 3% un und under der th der the he NZ NZ Copy CCopyright opy pyrig ight ht Act At Act. ...
Worksheet: Acid base problems - AP level
... of a 0.200 M acetic acid solution to make a buffer with pH = 5.000? Solution: 1) Use H-H Equation to determine required ratio of acetate to acid in solution: 5.000 = 4.752 + log [base] /[acid] log [base] /[acid] = 0.248 [base] /[acid] = 1.77 2) Determine molar amount of base required to get pH = 5.0 ...
... of a 0.200 M acetic acid solution to make a buffer with pH = 5.000? Solution: 1) Use H-H Equation to determine required ratio of acetate to acid in solution: 5.000 = 4.752 + log [base] /[acid] log [base] /[acid] = 0.248 [base] /[acid] = 1.77 2) Determine molar amount of base required to get pH = 5.0 ...
Chemical Energy
... The common sense tells us that the formation of a though d are exothermic. Check the standard enthalpy of formation. A lot of energy is required to break the triple bond in 0.5 N2 + O2 - NO2 ...
... The common sense tells us that the formation of a though d are exothermic. Check the standard enthalpy of formation. A lot of energy is required to break the triple bond in 0.5 N2 + O2 - NO2 ...
Thermochemistry
... 5. Construct a Born-Haber cycle for group 1 and group 2 oxides and chlorides, and use it to calculate an enthalpy change (9.1.12.A.1, 9.1.12.B.1) 6· Discuss the difference between theoretical and experimental lattice enthalpy values of ionic compounds in terms of their covalent character ...
... 5. Construct a Born-Haber cycle for group 1 and group 2 oxides and chlorides, and use it to calculate an enthalpy change (9.1.12.A.1, 9.1.12.B.1) 6· Discuss the difference between theoretical and experimental lattice enthalpy values of ionic compounds in terms of their covalent character ...
final review cp2 1213 by chapter
... 1.Which of the following explains why methane (CH4) has a boiling point of – 161 °C and octane (C8H18) has a boiling point of 125.6 °C. A.the London dispersion forces are stronger in methane B.the hydrogen bonds are stronger in octane C.octane can hydrogen bond and methane cannot D.the hydrogen bond ...
... 1.Which of the following explains why methane (CH4) has a boiling point of – 161 °C and octane (C8H18) has a boiling point of 125.6 °C. A.the London dispersion forces are stronger in methane B.the hydrogen bonds are stronger in octane C.octane can hydrogen bond and methane cannot D.the hydrogen bond ...
Document
... 1. The standard state of a pure gases substance, denoted by g, at a given temperature is the ideal gas at 1 bar pressure. 2. The standard state of a pure liquid substance, denoted by l, at a given temperature is the pure liquid at 1 bar pressure. 3. The standard state of a pure crystalline substance ...
... 1. The standard state of a pure gases substance, denoted by g, at a given temperature is the ideal gas at 1 bar pressure. 2. The standard state of a pure liquid substance, denoted by l, at a given temperature is the pure liquid at 1 bar pressure. 3. The standard state of a pure crystalline substance ...
Unit 2:
... pH of the reaction mixture. The mole ratio of oxidizing to reducing agent is two to five at pH 1, and is two to one at pH 13. For each of these cases, write a balanced equation for the reaction, and indicate the oxidation state of the manganese in the product containing manganese. 1981 B A 1.2516 gr ...
... pH of the reaction mixture. The mole ratio of oxidizing to reducing agent is two to five at pH 1, and is two to one at pH 13. For each of these cases, write a balanced equation for the reaction, and indicate the oxidation state of the manganese in the product containing manganese. 1981 B A 1.2516 gr ...
Molarity = M (Concentration of Solutions)
... Gas Law Stoichiometry - I - NH3 + HCl Problem: A slide separating two containers is removed, and the gases are allowed to mix and react. The first container with a volume of 2.79 L contains Ammonia gas at a pressure of 0.776 atm and a temperature of 18.7 oC. The second with a volume of 1.16 L conta ...
... Gas Law Stoichiometry - I - NH3 + HCl Problem: A slide separating two containers is removed, and the gases are allowed to mix and react. The first container with a volume of 2.79 L contains Ammonia gas at a pressure of 0.776 atm and a temperature of 18.7 oC. The second with a volume of 1.16 L conta ...
Preparation of spherical DDNP study Liu off on a journey
... Influence of ammonia salt crystals diazotization due in ammonia salt filtration process Amount drained liquor, ammonium salt crystals when stout, filtration fast, do not And then washed with water. Because the sodium picramate reduction is an exothermic reaction, the addition point may be scattered ...
... Influence of ammonia salt crystals diazotization due in ammonia salt filtration process Amount drained liquor, ammonium salt crystals when stout, filtration fast, do not And then washed with water. Because the sodium picramate reduction is an exothermic reaction, the addition point may be scattered ...
Document
... • Suppose the system is in equilibrium at 300°C, and you increase the temperature to 500°C. How can the reaction counteract the change you have made? How can it cool itself down again? • To cool down, it needs to absorb the extra heat that you have just put in. In the case we are looking at, the bac ...
... • Suppose the system is in equilibrium at 300°C, and you increase the temperature to 500°C. How can the reaction counteract the change you have made? How can it cool itself down again? • To cool down, it needs to absorb the extra heat that you have just put in. In the case we are looking at, the bac ...
College Chemistry I PHS 1025 Fall 2012 Practice Exam 3A
... containing 500. g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is 4.18 J/(g ∙ °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene. A) -7070 kJ/mol B) +39.7 kJ/mol C) -81 ...
... containing 500. g of water, the temperature of the water increases by 8.63°C. Assuming that the specific heat of water is 4.18 J/(g ∙ °C), and that the heat absorption by the calorimeter is negligible, estimate the enthalpy of combustion per mole of anthracene. A) -7070 kJ/mol B) +39.7 kJ/mol C) -81 ...
Powerpoint
... For a chemical reaction, Ho is usually reported at specific temperature, e.g., for the reaction C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(l) Ho298K is the enthalpy change when C6H12O6(s) and O2(g) at 298K are converted to CO2(g) and H2O(l) at 298K. Ho273K is the enthalpy change when C6H12O6(s) and O2( ...
... For a chemical reaction, Ho is usually reported at specific temperature, e.g., for the reaction C6H12O6(s) + 6O2(g) 6CO2(g) + 6H2O(l) Ho298K is the enthalpy change when C6H12O6(s) and O2(g) at 298K are converted to CO2(g) and H2O(l) at 298K. Ho273K is the enthalpy change when C6H12O6(s) and O2( ...
Reliability and Improvements of Water Titration by the Karl Fischer
... reasonable conformance only for the wet sample C. For the rather dry samples A and B only a trend is recognizable. Systematic differences are obvious. It has to be mentioned, that at dry oils the results also scatter within one single laboratory, a standard deviation of 20 % is not unusual. The foll ...
... reasonable conformance only for the wet sample C. For the rather dry samples A and B only a trend is recognizable. Systematic differences are obvious. It has to be mentioned, that at dry oils the results also scatter within one single laboratory, a standard deviation of 20 % is not unusual. The foll ...
07 Aromatic compounds. Acids of arom.s.,their salts, esters,amides
... interesting from the standpoint of being considerably less toxic than aniline. The para-compounds (C-3) is of particular interast from two standpoint: namely it is the metabolic product of aniline, and it is the least toxic of the three possible aminophenols. It also possesses a strong antipyretic a ...
... interesting from the standpoint of being considerably less toxic than aniline. The para-compounds (C-3) is of particular interast from two standpoint: namely it is the metabolic product of aniline, and it is the least toxic of the three possible aminophenols. It also possesses a strong antipyretic a ...
Thermometric titration
A thermometric titration is one of a number of instrumental titration techniques where endpoints can be located accurately and precisely without a subjective interpretation on the part of the analyst as to their location. Enthalpy change is arguably the most fundamental and universal property of chemical reactions, so the observation of temperature change is a natural choice in monitoring their progress. It is not a new technique, with possibly the first recognizable thermometric titration method reported early in the 20th century (Bell and Cowell, 1913). In spite of its attractive features, and in spite of the considerable research that has been conducted in the field and a large body of applications that have been developed; it has been until now an under-utilized technique in the critical area of industrial process and quality control. Automated potentiometric titration systems have pre-dominated in this area since the 1970s. With the advent of cheap computers able to handle the powerful thermometric titration software, development has now reached the stage where easy to use automated thermometric titration systems can in many cases offer a superior alternative to potentiometric titrimetry.The applications of thermometric titrimetry discussed on this page are by no means exhaustive. The reader is referred to the bibliography for further reading on the subject.