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 ...
Heat of reaction
... their standard state produce products in their standard state is called the standard enthalpy of reaction (ΔH°). • The standard state of a substance is its pure and most stable form at 1 atmosphere pressure and at 25°C. • The enthalpy change for the formation of one mole of a compound in its standar ...
... their standard state produce products in their standard state is called the standard enthalpy of reaction (ΔH°). • The standard state of a substance is its pure and most stable form at 1 atmosphere pressure and at 25°C. • The enthalpy change for the formation of one mole of a compound in its standar ...
Advanced Placement Chemistry
... (C) all points on the curve between Q and S (D) all points on the curve between R and T (E) no point on the curve . . .C10H12O4S(s) + . . O2(g) ---> . . . CO2(g) + . . . SO2(g) + . . . H2O(g) 26. When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms, ...
... (C) all points on the curve between Q and S (D) all points on the curve between R and T (E) no point on the curve . . .C10H12O4S(s) + . . O2(g) ---> . . . CO2(g) + . . . SO2(g) + . . . H2O(g) 26. When the equation above is balanced and all coefficients are reduced to their lowest whole-number terms, ...
Chapter 4: Chemical Quantities and Aqueous Reactions
... • In a titration, one reactant (the titrant) is placed in a buret. The other reactant is placed in a flask along with a few drops of an indicator. • The titrant is slowly added to the contents of the flask until the indicator changes color (the endpoint). • If the indicator has been chosen properly, ...
... • In a titration, one reactant (the titrant) is placed in a buret. The other reactant is placed in a flask along with a few drops of an indicator. • The titrant is slowly added to the contents of the flask until the indicator changes color (the endpoint). • If the indicator has been chosen properly, ...
spring semester review
... 50. If the entropy change for the reaction below at 298 K and 1 atm pressure is 137 J/K, and S=205 J/mol x K for O 2(g), what is S for O3(g)? 2O3 ----> 3O2 a) 364 J/mol x K b) 478 J/mol x K c) 239 J/mol x K d) -117 J/mol x K e) -59 J/mol x K 51.Which one on the following reactions has a positive ent ...
... 50. If the entropy change for the reaction below at 298 K and 1 atm pressure is 137 J/K, and S=205 J/mol x K for O 2(g), what is S for O3(g)? 2O3 ----> 3O2 a) 364 J/mol x K b) 478 J/mol x K c) 239 J/mol x K d) -117 J/mol x K e) -59 J/mol x K 51.Which one on the following reactions has a positive ent ...
Chemistry 1A Final Exam December 12, 2001 Page 1 of 16 (Closed
... Part I Multiple Choice (5 pts each, 225 pts total) Bubble in the correct answer on your ScantronTM form AND circle your answer on the exam. There is only one correct answer for each question, so you should circle and fill in one and only one answer for each question. There is no penalty for an incor ...
... Part I Multiple Choice (5 pts each, 225 pts total) Bubble in the correct answer on your ScantronTM form AND circle your answer on the exam. There is only one correct answer for each question, so you should circle and fill in one and only one answer for each question. There is no penalty for an incor ...
Water: The Universal Solvent
... mass, what additional information is necessary to calculate the molarity of the solution? I. The density of water II. The density of the solution III. The molar mass of sucrose (A) I only (B) II only (C) III only (D) I and III (E) II and III ...
... mass, what additional information is necessary to calculate the molarity of the solution? I. The density of water II. The density of the solution III. The molar mass of sucrose (A) I only (B) II only (C) III only (D) I and III (E) II and III ...
Project Advance Chemistry 106 Sample Questions
... 36. Given Ka values of 5.6 × 10-10 and 4.8 × 10-10 for NH4+ and HCN respectively, calculate the equilibrium constant for the following reaction. NH4+ + CNA. B. C. D. E. ...
... 36. Given Ka values of 5.6 × 10-10 and 4.8 × 10-10 for NH4+ and HCN respectively, calculate the equilibrium constant for the following reaction. NH4+ + CNA. B. C. D. E. ...
Time
... 4 HCl (g) + O2(g) 2 H2O(g) + 2 Cl2(g) + 113 kJ What effect would the following changes have on the equilibrium concentration of Cl2? i) increasing the temperature of the system ii) decreasing the total pressure on the system iii) increasing the concentration of oxygen gas iv) adding a catalyst ...
... 4 HCl (g) + O2(g) 2 H2O(g) + 2 Cl2(g) + 113 kJ What effect would the following changes have on the equilibrium concentration of Cl2? i) increasing the temperature of the system ii) decreasing the total pressure on the system iii) increasing the concentration of oxygen gas iv) adding a catalyst ...
Spring 2002 - Kwantlen Polytechnic University
... Avogadro’s number = 6.02 x 1023 Faraday = 96485 Coulombs R = 0.08206 L-atm/mol-K = 8.314 J/mol-K Arrhenius equation: k = Ae-Ea/RT Nernst equation: ε = ε° - (0.05916/n)log Q (at 25°C) First order kinetics: ln(Ao/A) = kt Second order kinetics: [1/A] - [1/Ao] = kt Freezing point depression and boiling ...
... Avogadro’s number = 6.02 x 1023 Faraday = 96485 Coulombs R = 0.08206 L-atm/mol-K = 8.314 J/mol-K Arrhenius equation: k = Ae-Ea/RT Nernst equation: ε = ε° - (0.05916/n)log Q (at 25°C) First order kinetics: ln(Ao/A) = kt Second order kinetics: [1/A] - [1/Ao] = kt Freezing point depression and boiling ...
Oxidation-Reduction Reactions Oxidation-Reduction
... The concentration of aqueous I3- solution can be determined by titration with aqueous sodium thiosulfate, Na2S2O3. What is the molarity of I3- if 24.55 mL of 0.102 M Na2S2O3 is needed for complete reaction with 10.00 mL of the I3- solution? The net ionic equation is: 2 S2O32- (aq) + I3- (aq) S4O62- ...
... The concentration of aqueous I3- solution can be determined by titration with aqueous sodium thiosulfate, Na2S2O3. What is the molarity of I3- if 24.55 mL of 0.102 M Na2S2O3 is needed for complete reaction with 10.00 mL of the I3- solution? The net ionic equation is: 2 S2O32- (aq) + I3- (aq) S4O62- ...
Equilibrium Review worksheet
... In a rigid 1.00 L laboratory reaction vessel, a technician places 1.00 mol of each of the four substances involved in this equilibrium. The vessel is heated to 650 °C. Determine the equilibrium amount concentrations of each substance, organizing your values in an ICE table. (Hint: use the value of K ...
... In a rigid 1.00 L laboratory reaction vessel, a technician places 1.00 mol of each of the four substances involved in this equilibrium. The vessel is heated to 650 °C. Determine the equilibrium amount concentrations of each substance, organizing your values in an ICE table. (Hint: use the value of K ...
L1 – CHEMISTRY FINAL REVIEW
... 32. Describe the Van Der Waals forces between water molecules called dipole interactions or Hydrogen bonds. H-bond is a strong intermolecular bond between the slightly positive Hydrogen end of one water molecule and the slightly neg. oxygen end of an adjacent water molecule. 33. Name 4 unique proper ...
... 32. Describe the Van Der Waals forces between water molecules called dipole interactions or Hydrogen bonds. H-bond is a strong intermolecular bond between the slightly positive Hydrogen end of one water molecule and the slightly neg. oxygen end of an adjacent water molecule. 33. Name 4 unique proper ...
Making Connections - SCH4U1-CCVI
... Total energy of the universe is constant Energy cannot be created or destroyed, just transferred from one form to another For a chemical reaction ∆Hºuniverse = __________________________________________ In a chemical reaction, the PE of the reactants and products results in the transfer of energ ...
... Total energy of the universe is constant Energy cannot be created or destroyed, just transferred from one form to another For a chemical reaction ∆Hºuniverse = __________________________________________ In a chemical reaction, the PE of the reactants and products results in the transfer of energ ...
Reaction Systems Engineering II (part 1)
... hardly soluble salt well approximated by an ideal solution * Solubility difficult to measure can be calculated from the thermodynamic functions. ...
... hardly soluble salt well approximated by an ideal solution * Solubility difficult to measure can be calculated from the thermodynamic functions. ...
2015 Academic Challenge CHEMISTRY TEST – STATE
... ©2015 Worldwide Youth in Science and Engineering “WYSE”, “Worldwide Youth in Science and Engineering” and the “WYSE Design” are service marks of and this work is Copyright ©2015 by the Board of Trustees of the University of Illinois at Urbana – Champaign. All rights reserved ...
... ©2015 Worldwide Youth in Science and Engineering “WYSE”, “Worldwide Youth in Science and Engineering” and the “WYSE Design” are service marks of and this work is Copyright ©2015 by the Board of Trustees of the University of Illinois at Urbana – Champaign. All rights reserved ...
File
... 62. A 0.500 gram sample of a monoprotic acid is dissolved in water and 40.0 mL of 0.100 M NaOH is needed to titrate the sample to the equivalence point. What is the molar mass of the acid? A) 50.0 g B) 62.5 g C) 125 g D) 200 g E) 250 g 63. The pH of a solution prepared by adding 10.0 mL of 0.020 mol ...
... 62. A 0.500 gram sample of a monoprotic acid is dissolved in water and 40.0 mL of 0.100 M NaOH is needed to titrate the sample to the equivalence point. What is the molar mass of the acid? A) 50.0 g B) 62.5 g C) 125 g D) 200 g E) 250 g 63. The pH of a solution prepared by adding 10.0 mL of 0.020 mol ...
CHEM 30
... a) is this reaction exothermic or endothermic? b) how much heat will be released when 5.10 g of ammonia form? In an experiment using a simple styrofoam calorimeter, a student dissolves 4.62 g of KOH in 250 o o mL of distilled water. The temperature of the water increases from 21.6 C to 28.4 C Calcul ...
... a) is this reaction exothermic or endothermic? b) how much heat will be released when 5.10 g of ammonia form? In an experiment using a simple styrofoam calorimeter, a student dissolves 4.62 g of KOH in 250 o o mL of distilled water. The temperature of the water increases from 21.6 C to 28.4 C Calcul ...
2014 Academic Challenge Sectional Chemistry Exam Solution Set 1
... top of the hill. The activation energy of the reverse reaction is the distance from the products to the top of the hill. The exothermic nature of the reaction requires EAfwd to be less than EArev. It is not required that this obey a first order rate law or be a gas phase reaction (B or D). The disso ...
... top of the hill. The activation energy of the reverse reaction is the distance from the products to the top of the hill. The exothermic nature of the reaction requires EAfwd to be less than EArev. It is not required that this obey a first order rate law or be a gas phase reaction (B or D). The disso ...
king fahd university of petroleum and minerals chemistry
... 11. A 20.0 mL sample of 0.150 M ethylamine (CH3CH2NH2) is titrated with 0.0981 M HCl. What is the pH after the addition of 5.0 mL of HCl? For ethylamine, pKb = 3.25. A) B) C) D) ...
... 11. A 20.0 mL sample of 0.150 M ethylamine (CH3CH2NH2) is titrated with 0.0981 M HCl. What is the pH after the addition of 5.0 mL of HCl? For ethylamine, pKb = 3.25. A) B) C) D) ...
97KB - NZQA
... The colourless solution of hydrogen peroxide, when black MnO2 is added, would produce a colourless liquid of water, and bubbles of colourless oxygen gas would form and it would get warm. This reaction is a decomposition reaction, as a single reactant (hydrogen peroxide) forms two products (water and ...
... The colourless solution of hydrogen peroxide, when black MnO2 is added, would produce a colourless liquid of water, and bubbles of colourless oxygen gas would form and it would get warm. This reaction is a decomposition reaction, as a single reactant (hydrogen peroxide) forms two products (water and ...
Honors-Final-Review-2014
... _____1. Ionic bond _____2. Covalent bond _____3. polar covalent _____4. nonpolar covalent _____5. sigma bond _____6. pi bond _____7. resonance structures _____8. multiple covalent bonds _____9. octet rule _____10. VSEPR Chapter 9 Stoichiometry _____ 1. Reaction Stoich _____ 2. Theoretical Yield ____ ...
... _____1. Ionic bond _____2. Covalent bond _____3. polar covalent _____4. nonpolar covalent _____5. sigma bond _____6. pi bond _____7. resonance structures _____8. multiple covalent bonds _____9. octet rule _____10. VSEPR Chapter 9 Stoichiometry _____ 1. Reaction Stoich _____ 2. Theoretical Yield ____ ...
Final Review
... a. The molarity of a solution containing 42.6g of sodium hydroxide in 3.00L of water. b. The number of moles of solute present in 680mL of a 0.25M Na2SO4 solution. c. The number of grams of KBr present in 500mL of a 0.100 M solution. 5. Describe how to prepare the following solutions. Include calcul ...
... a. The molarity of a solution containing 42.6g of sodium hydroxide in 3.00L of water. b. The number of moles of solute present in 680mL of a 0.25M Na2SO4 solution. c. The number of grams of KBr present in 500mL of a 0.100 M solution. 5. Describe how to prepare the following solutions. Include calcul ...
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.