1 Q. If ΔrH is positive, what can you say about the reaction? 2 Q If
... 9 Q For the reaction C(s) + O2(g) Æ CO2(g) ΔrH = -400 kJ/ mol-1. How much heat would be released when 88 g of CO2 is produced? Where do we commonly see this reaction used? ...
... 9 Q For the reaction C(s) + O2(g) Æ CO2(g) ΔrH = -400 kJ/ mol-1. How much heat would be released when 88 g of CO2 is produced? Where do we commonly see this reaction used? ...
experiment 10 - Faculty Web Pages
... where A, B, C, and D all exist as ions in solution. Will a reaction happen, and if so, what will be the products? Each of the positive ions could combine with the negative ion of the other compound, i.e. A+ and D¯ and C+ and B¯. The formation of a precipitate, the evolution of a gas, and a temperatu ...
... where A, B, C, and D all exist as ions in solution. Will a reaction happen, and if so, what will be the products? Each of the positive ions could combine with the negative ion of the other compound, i.e. A+ and D¯ and C+ and B¯. The formation of a precipitate, the evolution of a gas, and a temperatu ...
Semester 2 Review
... A. How will an increase in temperature change the concentration of hydrogen gas? ________ B. How will an increase in pressure affect the system? ___________________ C. Which direction will the addition of iodine gas shift the system? _________________ What does this do to the concentration of hydrog ...
... A. How will an increase in temperature change the concentration of hydrogen gas? ________ B. How will an increase in pressure affect the system? ___________________ C. Which direction will the addition of iodine gas shift the system? _________________ What does this do to the concentration of hydrog ...
Answer Key to Sample Questions
... positive because one molecule breaks to form two molecules b. What is the sign of H for this reaction? positive because a bond is broken, but none is formed. c. In which temperature range will this reaction be thermodynamically favored? It is entropy favored, enthalpy disfavored, so favored overall ...
... positive because one molecule breaks to form two molecules b. What is the sign of H for this reaction? positive because a bond is broken, but none is formed. c. In which temperature range will this reaction be thermodynamically favored? It is entropy favored, enthalpy disfavored, so favored overall ...
nomenclature review
... ________ Magnesium chloride is dissolved in water. ________ Hydrochloric acid neutralizes sodium hydroxide to form sodium chloride and water. 13. Why are phase changes considered only physical changes? 14. Sketch an example of the following at the molecular level: a. a gaseous compound b. a mixture ...
... ________ Magnesium chloride is dissolved in water. ________ Hydrochloric acid neutralizes sodium hydroxide to form sodium chloride and water. 13. Why are phase changes considered only physical changes? 14. Sketch an example of the following at the molecular level: a. a gaseous compound b. a mixture ...
Chemistry 30 Notes - Heat of Formation February 2nd
... What determines whether a reaction will actually occur spontaneously or not? In chemistry, a "spontaneous" reaction is a reaction that will occur on its own - it may be fast or it may be slow. Here are some examples of spontaneous chemical reactions: Na(s) + ½Cl2(g) → NaCl(s) + 411.2 kJ H2(g) + ½O2( ...
... What determines whether a reaction will actually occur spontaneously or not? In chemistry, a "spontaneous" reaction is a reaction that will occur on its own - it may be fast or it may be slow. Here are some examples of spontaneous chemical reactions: Na(s) + ½Cl2(g) → NaCl(s) + 411.2 kJ H2(g) + ½O2( ...
Chemistry 520 - Problem Set 6
... 7. At 298 K the standard enthalpy of combustion of sucrose is -5645 kJ/mol and the standard Gibbs free energy of the reaction is -5797 kJ/mol. Estimate the additional non-expansion work that may be obtained by raising the temperature to blood temperature, 37C. ...
... 7. At 298 K the standard enthalpy of combustion of sucrose is -5645 kJ/mol and the standard Gibbs free energy of the reaction is -5797 kJ/mol. Estimate the additional non-expansion work that may be obtained by raising the temperature to blood temperature, 37C. ...
CHEMISTRY 1710 - Practice Exam #2
... gaseous CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is 0.857 J/(g · °C), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol. ...
... gaseous CCl4 at 76.8°C (the normal boiling point for CCl4). The specific heat of CCl4(l) is 0.857 J/(g · °C), its heat of fusion is 3.27 kJ/mol, and its heat of vaporization is 29.82 kJ/mol. ...
exam review - hrsbstaff.ednet.ns.ca
... *10. Calculate ΔG at 25°C for the following reaction, by first calculating ΔH and ΔS. Once you've found ΔH and ΔS, solve for ΔG using the formula: ΔG = ΔH - T ΔS Also - will this reaction be spontaneous at this temperature? CH3CO2H (l) + 2 O2 (g) → 2 CO2 (g) + 2 H2O (g) ...
... *10. Calculate ΔG at 25°C for the following reaction, by first calculating ΔH and ΔS. Once you've found ΔH and ΔS, solve for ΔG using the formula: ΔG = ΔH - T ΔS Also - will this reaction be spontaneous at this temperature? CH3CO2H (l) + 2 O2 (g) → 2 CO2 (g) + 2 H2O (g) ...
Self-Test Worksheet for Thermodynamics Section (Quiz
... measures the pool temperature to be 0 °C. He then runs the heater to warm the pool up to 30 °C. The heater costs $1 per min to run and it supplies 200,000 kJ of heat per minute (heat capacity of water is 4.18 J/g/°C, ∆Hfusion for water = 6.01 kJ/mol). (a) How much heat energy does the owner use? (b) ...
... measures the pool temperature to be 0 °C. He then runs the heater to warm the pool up to 30 °C. The heater costs $1 per min to run and it supplies 200,000 kJ of heat per minute (heat capacity of water is 4.18 J/g/°C, ∆Hfusion for water = 6.01 kJ/mol). (a) How much heat energy does the owner use? (b) ...
Answers PRACTICE EXAM II Spring 2008 Part I. Multiple Choice (3
... 8. Which one of the following best describes what occurs in a reaction system when it reaches a state of dynamic equilibrium? 4. the rates for both forward and reverse reaction processes are the same 9. Which of the following solutions has the lowest freezing point? 3. 1.0 m Na2SO4 in water 10. Ide ...
... 8. Which one of the following best describes what occurs in a reaction system when it reaches a state of dynamic equilibrium? 4. the rates for both forward and reverse reaction processes are the same 9. Which of the following solutions has the lowest freezing point? 3. 1.0 m Na2SO4 in water 10. Ide ...
A.P. Chemistry
... Calculations using Titration Data: M1V1 = M2V2 M = mol/L Volume in liters (be sure to convert mL L) (p. 145-147) Problem: What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H2SO4 solution? ...
... Calculations using Titration Data: M1V1 = M2V2 M = mol/L Volume in liters (be sure to convert mL L) (p. 145-147) Problem: What volume of 16 M sulfuric acid must be used to prepare 1.5 L of a 0.10 M H2SO4 solution? ...
Acid-Base Reactions
... 13. Label each as strong, weak or non electrolyte: CaCl2 strong electrolyte (ionic compound) HNO3 strong electrolyte (strong acid) C2H5OH (ethanol) nonelectrolyte (molecular compound, not acid/base) HCOOH (formic acid) weak electrolyte (weak acid) KOH strong electrolyte (ionic compound) Ca(NO3)2 (ca ...
... 13. Label each as strong, weak or non electrolyte: CaCl2 strong electrolyte (ionic compound) HNO3 strong electrolyte (strong acid) C2H5OH (ethanol) nonelectrolyte (molecular compound, not acid/base) HCOOH (formic acid) weak electrolyte (weak acid) KOH strong electrolyte (ionic compound) Ca(NO3)2 (ca ...
CH 301 Practice Test Questions
... mL flask. At 371 K, the pressure of the vapor in the flask is 754 torr. What is the molar mass in g/mol? 6. What is the density of nitrogen gas at STP? 7. Consider two equal-sized containers, one filled with H2 gas and one with O2 gas at the same temperature and pressure. The average velocity of the ...
... mL flask. At 371 K, the pressure of the vapor in the flask is 754 torr. What is the molar mass in g/mol? 6. What is the density of nitrogen gas at STP? 7. Consider two equal-sized containers, one filled with H2 gas and one with O2 gas at the same temperature and pressure. The average velocity of the ...
standard sample test
... 13. In the reaction of iron with nitric acid to form iron (II) nitrate and hydrogen gas (H2), if 1 mole of iron were to be reacted with 1 mole of nitric acid, how many moles of iron (II) nitrate would form? (a) 0.5 mole (b) 1 mole (c) 1.5 mole ...
... 13. In the reaction of iron with nitric acid to form iron (II) nitrate and hydrogen gas (H2), if 1 mole of iron were to be reacted with 1 mole of nitric acid, how many moles of iron (II) nitrate would form? (a) 0.5 mole (b) 1 mole (c) 1.5 mole ...
Thermodynamics Test Study Guide—AP _____ 1. The entropy
... bomb calorimeter that has a heat capacity of 2.510 kJ/oC. What is the internal energy change, per mole, of ethane for the combustion reaction? ______12. It is found that Go = -394 kJ/mole at a given temperature for the reaction: C(s) + O2(g) CO2(g) At this temperature, which statement is TRUE fo ...
... bomb calorimeter that has a heat capacity of 2.510 kJ/oC. What is the internal energy change, per mole, of ethane for the combustion reaction? ______12. It is found that Go = -394 kJ/mole at a given temperature for the reaction: C(s) + O2(g) CO2(g) At this temperature, which statement is TRUE fo ...
Are You suprised ?
... pressure of 0.329 atm at 35oC. At this temperature, the vapor pressure of pure acetone is 0.453 atm, and the vapor pressure of pure chloroform is 0.388 atm. By comparing the measured vapor pressure and the calculated one, the above solution is: A) Endothermic solution ...
... pressure of 0.329 atm at 35oC. At this temperature, the vapor pressure of pure acetone is 0.453 atm, and the vapor pressure of pure chloroform is 0.388 atm. By comparing the measured vapor pressure and the calculated one, the above solution is: A) Endothermic solution ...
AP Review Chp 1 and Chp 2 Wed 10/9/2013 1. Near room
... I) Magnesium displaces copper from a dilute solution of copper ( II) sulfate; the pure copper will settle out of the solution. Mg(s) + CuSO4(aq) MgSO4(aq) + Cu(s) A copper(II) sulfate solution is mixed by dissolving 25.000 g of copper(II) sulfate, and then it is treated with an excess of magnesium ...
... I) Magnesium displaces copper from a dilute solution of copper ( II) sulfate; the pure copper will settle out of the solution. Mg(s) + CuSO4(aq) MgSO4(aq) + Cu(s) A copper(II) sulfate solution is mixed by dissolving 25.000 g of copper(II) sulfate, and then it is treated with an excess of magnesium ...
CHEM_2nd_Semester_Final_R eview
... 16. How do gases create pressure, use KMT to support your answer. 17. Explain diffusion, use KMT to support your answer. 18. Is Boyle’s law direct or inverse? Charles’s Law? Gay-Lussac’s Law? 19. If 735 L of a gas is at 3.11 atm and 34 oC, what is its temperature at 6.11 atm and 235 L? 20. If 12.2 m ...
... 16. How do gases create pressure, use KMT to support your answer. 17. Explain diffusion, use KMT to support your answer. 18. Is Boyle’s law direct or inverse? Charles’s Law? Gay-Lussac’s Law? 19. If 735 L of a gas is at 3.11 atm and 34 oC, what is its temperature at 6.11 atm and 235 L? 20. If 12.2 m ...
Chemistry 2nd Semester Final Exam Review Chemical Bonds Give
... 16. How do gases create pressure, use KMT to support your answer. 17. Explain diffusion, use KMT to support your answer. 18. Is Boyle’s law direct or inverse? Charles’s Law? Gay-Lussac’s Law? 19. If 735 L of a gas is at 3.11 atm and 34 oC, what is its temperature at 6.11 atm and 235 L? 20. If 12.2 m ...
... 16. How do gases create pressure, use KMT to support your answer. 17. Explain diffusion, use KMT to support your answer. 18. Is Boyle’s law direct or inverse? Charles’s Law? Gay-Lussac’s Law? 19. If 735 L of a gas is at 3.11 atm and 34 oC, what is its temperature at 6.11 atm and 235 L? 20. If 12.2 m ...
2nd Semester Final Review
... 16. How do gases create pressure, use KMT to support your answer. 17. Explain diffusion, use KMT to support your answer. 18. Is Boyle’s law direct or inverse? Charles’s Law? Gay-Lussac’s Law? 19. If 735 L of a gas is at 3.11 atm and 34 oC, what is its temperature at 6.11 atm and 235 L? 20. If 12.2 m ...
... 16. How do gases create pressure, use KMT to support your answer. 17. Explain diffusion, use KMT to support your answer. 18. Is Boyle’s law direct or inverse? Charles’s Law? Gay-Lussac’s Law? 19. If 735 L of a gas is at 3.11 atm and 34 oC, what is its temperature at 6.11 atm and 235 L? 20. If 12.2 m ...
Thermochemistry
... Calorimetry is the science of measuring the heat of chemical reactions or physical changes. ...
... Calorimetry is the science of measuring the heat of chemical reactions or physical changes. ...
The bombardier beetle uses an explosive discharge as a defensive
... 5. A student performs an experiment to determine the molar enthalpy of solution of urea, H2NCONH2. The student place 91.95 g of water at 25oC into a coffee-cup calorimeter and immerses a thermometer in the water. After 50 s, the student adds 5.13 g of solid urea, also at 25oC, to the water and meas ...
... 5. A student performs an experiment to determine the molar enthalpy of solution of urea, H2NCONH2. The student place 91.95 g of water at 25oC into a coffee-cup calorimeter and immerses a thermometer in the water. After 50 s, the student adds 5.13 g of solid urea, also at 25oC, to the water and meas ...
Midterm 1 2009 (PDF format)
... b) The enthalpy change for a reaction is independent of the state of the reactants and products. c) Enthalpy is a state function. d) H is the value of q measured under conditions of constant volume. e) The enthalpy change of a reaction is the reciprocal of the ∆H of the reverse reaction. ...
... b) The enthalpy change for a reaction is independent of the state of the reactants and products. c) Enthalpy is a state function. d) H is the value of q measured under conditions of constant volume. e) The enthalpy change of a reaction is the reciprocal of the ∆H of the reverse reaction. ...
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.