problem 8 on 2003B exam
... 4. Write the formulas to show the reactants and the products for any FIVE of the laboratory situations described below. Answers to more than five choices will not be graded. In all cases, a reaction occurs. Assume that solutions are aqueous unless otherwise indicated. Represent substances in solutio ...
... 4. Write the formulas to show the reactants and the products for any FIVE of the laboratory situations described below. Answers to more than five choices will not be graded. In all cases, a reaction occurs. Assume that solutions are aqueous unless otherwise indicated. Represent substances in solutio ...
JF Physical Chemistry 2010-2011. JF CH 1101: Introduction to
... a. What is the internal energy U and the enthalpy H of a system? Write down an expression for the First Law of Thermodynamics which relates the change in internal energy of a system to the work done on the system and the heat absorbed by the system. Hence derive a relationship between the change in ...
... a. What is the internal energy U and the enthalpy H of a system? Write down an expression for the First Law of Thermodynamics which relates the change in internal energy of a system to the work done on the system and the heat absorbed by the system. Hence derive a relationship between the change in ...
No Slide Title
... Al2(SO4)3(aq) + 6NaOH(aq) → 2Al(OH)3(s) + 3Na2SO4(aq) *Do not carry the subscripts over (except for polyatomic ions) 2. Write the ionic equation showing the soluble product dissociated into ions, but the insoluble product left together. 2Al+3 + 3SO4-2 + 6Na+ + 6OH- → 2Al(OH)3(s) + 6Na+ + 3SO4-2 3. C ...
... Al2(SO4)3(aq) + 6NaOH(aq) → 2Al(OH)3(s) + 3Na2SO4(aq) *Do not carry the subscripts over (except for polyatomic ions) 2. Write the ionic equation showing the soluble product dissociated into ions, but the insoluble product left together. 2Al+3 + 3SO4-2 + 6Na+ + 6OH- → 2Al(OH)3(s) + 6Na+ + 3SO4-2 3. C ...
2009
... Two identical samples of copper(II) carbonate were added to an excess of 1 mol l–1 hydrochloric acid and 1 mol l–1 sulphuric acid respectively. Which of the following would have been different for the two reactions? A The pH of the final solution B ...
... Two identical samples of copper(II) carbonate were added to an excess of 1 mol l–1 hydrochloric acid and 1 mol l–1 sulphuric acid respectively. Which of the following would have been different for the two reactions? A The pH of the final solution B ...
Final Exam Review Sheets
... 6. Use collision theory to explain the effect of each factor below on the rate of a chemical reaction: a. temperature: An increase in temperature results in an increase in average kinetic energy of reactants. This means there will be an increase in the number of successful collisions between reactan ...
... 6. Use collision theory to explain the effect of each factor below on the rate of a chemical reaction: a. temperature: An increase in temperature results in an increase in average kinetic energy of reactants. This means there will be an increase in the number of successful collisions between reactan ...
Chapter 4: Aqueous Reactions and Solution
... develop the ability to recognize an acid, a base and an ionic compound from their formulas. An understanding of the nature of strong, weak and non-electrolytes in water is also needed. For oxidation-reduction reactions, you will need to become proficient at the use of the activity series. Larson-Foo ...
... develop the ability to recognize an acid, a base and an ionic compound from their formulas. An understanding of the nature of strong, weak and non-electrolytes in water is also needed. For oxidation-reduction reactions, you will need to become proficient at the use of the activity series. Larson-Foo ...
Chemistry Spell check on
... 1 Check that the answer sheet provided is for Chemistry Intermediate 2 (Section A). 2 For this section of the examination you must use an HB pencil and, where necessary, an eraser. 3 Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish Candidate Number ...
... 1 Check that the answer sheet provided is for Chemistry Intermediate 2 (Section A). 2 For this section of the examination you must use an HB pencil and, where necessary, an eraser. 3 Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish Candidate Number ...
Chapter 4. Aqueous Reactions and Solution Stoichiometry
... We sometimes have a problem with the arbitrary difference between strong and weak electrolytes. We often think that nonelectrolytes produce no ions in aqueous solution at all. We sometimes cannot tell the difference between dissolution and dissociation. The symbols (equilibrium) and (resonance) ...
... We sometimes have a problem with the arbitrary difference between strong and weak electrolytes. We often think that nonelectrolytes produce no ions in aqueous solution at all. We sometimes cannot tell the difference between dissolution and dissociation. The symbols (equilibrium) and (resonance) ...
Unit 8 Test Review
... Activity Series of Metals – an invaluable aid to predicting the products of replacement reactions. Each element on the list replaces from a compound any of the elements below it. The larger the interval between elements, the more vigorous the reaction. ...
... Activity Series of Metals – an invaluable aid to predicting the products of replacement reactions. Each element on the list replaces from a compound any of the elements below it. The larger the interval between elements, the more vigorous the reaction. ...
Classifying Chemical Reactions by What Atoms Do
... 2 HNO3(aq) + Ca(OH)2(aq) ➜ Ca(NO3)2(aq) + 2 H2O(l) Note that the cation from the base combines with the anion from the acid to make the water soluble salt. The net ionic equation for an acid-base reaction is H+(aq) + OH-(aq) ➜ H2O(l) (as long as the salt that forms is soluble in water) ...
... 2 HNO3(aq) + Ca(OH)2(aq) ➜ Ca(NO3)2(aq) + 2 H2O(l) Note that the cation from the base combines with the anion from the acid to make the water soluble salt. The net ionic equation for an acid-base reaction is H+(aq) + OH-(aq) ➜ H2O(l) (as long as the salt that forms is soluble in water) ...
2000 us national chemistry olympiad
... This is a multiple-choice examination with four choices for each question. There is only one correct or best answer to each question. When you select your choice, blacken the corresponding space on the answer sheet with your pencil. Make a heavy full mark, but no stray marks. If you decide to change ...
... This is a multiple-choice examination with four choices for each question. There is only one correct or best answer to each question. When you select your choice, blacken the corresponding space on the answer sheet with your pencil. Make a heavy full mark, but no stray marks. If you decide to change ...
Matter and Measurement
... To indicate when the equivalence point has been reached, a very small amount of a chemical compound called an INDICATOR is added to the HCl solution, before the NaOH is added. At the equivalence point, all the HCl has reacted. Addition of a very small amount of NaOH results in a dramatic color chan ...
... To indicate when the equivalence point has been reached, a very small amount of a chemical compound called an INDICATOR is added to the HCl solution, before the NaOH is added. At the equivalence point, all the HCl has reacted. Addition of a very small amount of NaOH results in a dramatic color chan ...
g) Chemistry 30 - Mr. Jones LHS Science
... d. If C6H6 (g), were consumed instead of C6H6 (l), would you expect the magnitude of H to increase, decrease, or stay the same? Explain. ...
... d. If C6H6 (g), were consumed instead of C6H6 (l), would you expect the magnitude of H to increase, decrease, or stay the same? Explain. ...
Chemical Equilibrium Review Ch 13-14 2015
... 3. Hydrogen iodide, HI, decomposes at moderate temperatures according to the equation: 2HI(g) 2(g) + I2(g) The amount of I2 in the reaction mixture can be determined from the intensity of the violet color of I2…the more intense the color, the more I2 in the reaction vessel. When 4.00mol HI was pla ...
... 3. Hydrogen iodide, HI, decomposes at moderate temperatures according to the equation: 2HI(g) 2(g) + I2(g) The amount of I2 in the reaction mixture can be determined from the intensity of the violet color of I2…the more intense the color, the more I2 in the reaction vessel. When 4.00mol HI was pla ...
Carefully detach the last page. It is the Data Sheet.
... convert carbon dioxide, water and energy into glucose and oxygen. The process of photosynthesis can be represented by the following chemical equation. ...
... convert carbon dioxide, water and energy into glucose and oxygen. The process of photosynthesis can be represented by the following chemical equation. ...
1C - Edexcel
... 3 The halogens are elements in Group 7 of the Periodic Table. The halogens react with metals to form compounds called halides. Table 1 shows information about some halogens and their halides. ...
... 3 The halogens are elements in Group 7 of the Periodic Table. The halogens react with metals to form compounds called halides. Table 1 shows information about some halogens and their halides. ...
Introductory Chemistry I
... 1. 10 mL of 0.2 M NaOH solution is placed into a small beaker with a small amount of phenolphthalein. . If 0.1 M HCl is added dropwise: a. the solution will become red on the first mL added, then change to colorless after 5 mL have been added. b. the solution will become red after 20 mL have been ad ...
... 1. 10 mL of 0.2 M NaOH solution is placed into a small beaker with a small amount of phenolphthalein. . If 0.1 M HCl is added dropwise: a. the solution will become red on the first mL added, then change to colorless after 5 mL have been added. b. the solution will become red after 20 mL have been ad ...
Chapter 5 Chemical Equilibrium 1 State whether each of the
... For this reaction, Δn = 0, thus Kc = Kp = 0.090 And since Kp is dimensionless, so is Kc. 7. Liquid water is always in equilibrium with H+(aq) and OH¯(aq) ions according to the reaction H2O(l) ...
... For this reaction, Δn = 0, thus Kc = Kp = 0.090 And since Kp is dimensionless, so is Kc. 7. Liquid water is always in equilibrium with H+(aq) and OH¯(aq) ions according to the reaction H2O(l) ...
1442 Final Review
... 36. If the concentration of hydroxide ion in a certain solution is 5.8 x 10-3 M, what is the pH of the solution? a) 3.58 b) 10.42 *c) 11.76 d) 11.42 e) 2.24 37. What is the pH of 0.035 M HClO4? a) 2.65 b) 3.52 c) 2.35 *d) 1.46 e) 1.65 38. What is the pH of 0.025 M barium hydroxide? a) 1.30 b) 1.60 c ...
... 36. If the concentration of hydroxide ion in a certain solution is 5.8 x 10-3 M, what is the pH of the solution? a) 3.58 b) 10.42 *c) 11.76 d) 11.42 e) 2.24 37. What is the pH of 0.035 M HClO4? a) 2.65 b) 3.52 c) 2.35 *d) 1.46 e) 1.65 38. What is the pH of 0.025 M barium hydroxide? a) 1.30 b) 1.60 c ...
Summer Work
... Third Exercise: Writing the balanced ionic Equation, predict the products for the following solutions are combined. Circle the precipitate (if any), place a box around the spectator ions. a. potassium chloride(aq) + silver(I) nitrate(aq) → b. lead (II) nitrate(aq) + hydrogen chloride(aq) → c. sodium ...
... Third Exercise: Writing the balanced ionic Equation, predict the products for the following solutions are combined. Circle the precipitate (if any), place a box around the spectator ions. a. potassium chloride(aq) + silver(I) nitrate(aq) → b. lead (II) nitrate(aq) + hydrogen chloride(aq) → c. sodium ...
General Chemistry Questions
... 6. Two solutions (the system), each of 25.0 mL volume and at 25.0 °C, are mixed in a beaker. A reaction occurs between them, causing the temperature to drop to 20.0 °C. After the products have equilibrated with the surroundings, the temperature is again 25.0 °C and the total volume is 50.0 mL. No ga ...
... 6. Two solutions (the system), each of 25.0 mL volume and at 25.0 °C, are mixed in a beaker. A reaction occurs between them, causing the temperature to drop to 20.0 °C. After the products have equilibrated with the surroundings, the temperature is again 25.0 °C and the total volume is 50.0 mL. No ga ...
Chapter 14
... Section 14.2 to identify how their equilibrium constants are related. Multiplying the first equation by a constant factor of 3 gives the second equation. (1) N2H4 (g) + 4/3 ClF3 (g) ' 4 HF (g) + N2 (g) + 2/3 Cl2 (g) (2) 3 N2H4 (g) + 4 ClF3 (g) ' 12 HF (g) + 3 N2 (g) + 2 Cl2 (g) This change means we ...
... Section 14.2 to identify how their equilibrium constants are related. Multiplying the first equation by a constant factor of 3 gives the second equation. (1) N2H4 (g) + 4/3 ClF3 (g) ' 4 HF (g) + N2 (g) + 2/3 Cl2 (g) (2) 3 N2H4 (g) + 4 ClF3 (g) ' 12 HF (g) + 3 N2 (g) + 2 Cl2 (g) This change means we ...
Reactions in Aqueous Solution (Brown 13th-Fossum
... • Arrhenius: substances that increase the concentration of H+ when dissolved in water. • Brønsted and Lowry: proton donors. Bases – Taste bitter and have a high pH. (Turn litmus paper blue.) • Arrhenius: Increase the concentration of OH− when dissolved in water. • Brønsted and Lowry: proton acceptor ...
... • Arrhenius: substances that increase the concentration of H+ when dissolved in water. • Brønsted and Lowry: proton donors. Bases – Taste bitter and have a high pH. (Turn litmus paper blue.) • Arrhenius: Increase the concentration of OH− when dissolved in water. • Brønsted and Lowry: proton acceptor ...
153KB PDF - Clydeview Academy
... 2 For this section of the examination you must use an HB pencil and, where necessary, an eraser. 3 Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish Candidate Number) and Centre Name printed on it. Do not change any of these details. 4 If any of this informa ...
... 2 For this section of the examination you must use an HB pencil and, where necessary, an eraser. 3 Check that the answer sheet you have been given has your name, date of birth, SCN (Scottish Candidate Number) and Centre Name printed on it. Do not change any of these details. 4 If any of this informa ...
AP Chemistry Syllabus
... results mean. Graphs should have a title and labeled axes. 9. Post-lab Questions Same as pre-lab questions 10. Conclusion and Error Analysis This is not a summary of results or procedure. It must state what was learned, such as a scientific principle, based on the purpose of the lab. It also include ...
... results mean. Graphs should have a title and labeled axes. 9. Post-lab Questions Same as pre-lab questions 10. Conclusion and Error Analysis This is not a summary of results or procedure. It must state what was learned, such as a scientific principle, based on the purpose of the lab. It also include ...
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.