1996 Free Response Answers
... Hypochlorous acid, HOCl, is a weak acid commonly used as a bleaching agent. The aciddissociation constant, Ka, for the reaction represented above is 3.2 x 10¯8. (a) Calculate the [H+] of a 0.14-molar solution of HOCl. (b) Write the correctly balanced net ionic equation for the reaction that occurs ...
... Hypochlorous acid, HOCl, is a weak acid commonly used as a bleaching agent. The aciddissociation constant, Ka, for the reaction represented above is 3.2 x 10¯8. (a) Calculate the [H+] of a 0.14-molar solution of HOCl. (b) Write the correctly balanced net ionic equation for the reaction that occurs ...
Exam Review Chapter 18-Equilibrium
... 7. Two opposing reactions (A + B ↔C + D) occurring simultaneously at the same rate is an example of: a. reversibility. c. neither a nor b b. chemical equilibrium. d. both a and b 8. According to collision theory, in order for a chemical reaction to occur, the reactant atoms must: a. make contact wit ...
... 7. Two opposing reactions (A + B ↔C + D) occurring simultaneously at the same rate is an example of: a. reversibility. c. neither a nor b b. chemical equilibrium. d. both a and b 8. According to collision theory, in order for a chemical reaction to occur, the reactant atoms must: a. make contact wit ...
Form A 1 Chem 130 Name______________________________
... have a situation where we have a negative H and a negative S. Since G = H - TS, the spontaneity of the reaction will depend on temperature. In order for G to be negative and have a spontaneous reaction, temperature must be low in order for H - TS to remain negative. Therefore, we expect this ...
... have a situation where we have a negative H and a negative S. Since G = H - TS, the spontaneity of the reaction will depend on temperature. In order for G to be negative and have a spontaneous reaction, temperature must be low in order for H - TS to remain negative. Therefore, we expect this ...
AP CHEMISTRY PROBLEMS ENTHALPY, ENTROPY, AND FREE
... 7. When most biologic enzymes are heated, they lose their catalytic activity. The change Original enzyme new form that occurs on heating is endothermic and spontaneous. Is the structure of the original enzyme or its new form more ordered? Explain. ...
... 7. When most biologic enzymes are heated, they lose their catalytic activity. The change Original enzyme new form that occurs on heating is endothermic and spontaneous. Is the structure of the original enzyme or its new form more ordered? Explain. ...
SPRING 2002 Test 2 1. Which of the following statements is
... A. At equilibrium, the concentrations of all species are constant B. The value of the equilibrium constant depends on the temperature C. At equilibrium, the reaction has stopped D. At equilibrium, the forward and reverse reactions are happening at the same rate E. Pure solids are not included in the ...
... A. At equilibrium, the concentrations of all species are constant B. The value of the equilibrium constant depends on the temperature C. At equilibrium, the reaction has stopped D. At equilibrium, the forward and reverse reactions are happening at the same rate E. Pure solids are not included in the ...
Answers to Homework Problem Sheet 8
... The temperature change, ΔT = (31.1 °C – 24.6 °C) = 6.7 K. The heat capacity of water is 4.184 J K-1 g-1. The heat change is therefore: q = c × m × ΔT = (4.184 J K-1 g-1) × (199 g) × (6.7 K) = 5600 J or 5.6 kJ (heat released) The number of moles of H+ and OH- present are both the same: number of mole ...
... The temperature change, ΔT = (31.1 °C – 24.6 °C) = 6.7 K. The heat capacity of water is 4.184 J K-1 g-1. The heat change is therefore: q = c × m × ΔT = (4.184 J K-1 g-1) × (199 g) × (6.7 K) = 5600 J or 5.6 kJ (heat released) The number of moles of H+ and OH- present are both the same: number of mole ...
C 3 H 8 (g) - Ms Critchley`s Lab
... sulphate experiments you have done). • Bond enthalpies can also be used to estimate ΔHr ...
... sulphate experiments you have done). • Bond enthalpies can also be used to estimate ΔHr ...
Chemistry and the material world
... K = 1 means that the reaction quotient is balanced. There is approximately the same amount of educt and product in the reaction mixture. K > 1 means that that the numerator in the reaction quotient is larger. There is more product in the reaction mixture. K < 1 means that the denominator in the reac ...
... K = 1 means that the reaction quotient is balanced. There is approximately the same amount of educt and product in the reaction mixture. K > 1 means that that the numerator in the reaction quotient is larger. There is more product in the reaction mixture. K < 1 means that the denominator in the reac ...
Thermobest for Chem1
... Endothermic process is any process in which heat has to be supplied to the system from the surroundings. energy + 2HgO (s) energy + H2O (s) ...
... Endothermic process is any process in which heat has to be supplied to the system from the surroundings. energy + 2HgO (s) energy + H2O (s) ...
Fe(H2O)63+ + H2O → ← H3O+ + Fe(H2O)5(OH)2+
... 51. If a reaction proceeding by the mechanism A + B → C + D occurs at a rate x, and if the concentrations of A and B are both doubled, what will be the new rate of reaction? (A) (B) (C) (D) (E) ...
... 51. If a reaction proceeding by the mechanism A + B → C + D occurs at a rate x, and if the concentrations of A and B are both doubled, what will be the new rate of reaction? (A) (B) (C) (D) (E) ...
MULTIPLE CHOICE
... 7) The net ionic equation for the reaction between aqueous solutions of HF and KOH is __________. A) HF + KOH H2O + K+ + FB) HF + OH- H2O + FC) HF + K+ + OH- H2O + KF ...
... 7) The net ionic equation for the reaction between aqueous solutions of HF and KOH is __________. A) HF + KOH H2O + K+ + FB) HF + OH- H2O + FC) HF + K+ + OH- H2O + KF ...
Chemical Reaction Th..
... Here is the equations you can use to calculate the values of G°T and H°T from G°298 and H°298 ...
... Here is the equations you can use to calculate the values of G°T and H°T from G°298 and H°298 ...
CHEMSTRY FREE-RESPONSE QUESTIONS (Form B)
... V = the volume, in liters, of MnO4-(aq)) added to reach the end point In terms of these variables, the number of moles of MnO4-(aq)) added to reach the end point of the titration is expressed a M x V. Using the variables defined above the molar mass of iron (55.85 g mol-1) and the coefficients in th ...
... V = the volume, in liters, of MnO4-(aq)) added to reach the end point In terms of these variables, the number of moles of MnO4-(aq)) added to reach the end point of the titration is expressed a M x V. Using the variables defined above the molar mass of iron (55.85 g mol-1) and the coefficients in th ...
makeup6
... 28. If 40.0 mL of 0.20 M CH3COOH are titrated with 0.20 M NaOH, how many mL of base must be added to form a buffer solution with the greatest buffering capacity? (A) 5.0 (B) 10.0 (C) 20.0 (D) 40.0 ...
... 28. If 40.0 mL of 0.20 M CH3COOH are titrated with 0.20 M NaOH, how many mL of base must be added to form a buffer solution with the greatest buffering capacity? (A) 5.0 (B) 10.0 (C) 20.0 (D) 40.0 ...
chemistry important question i
... (iii) 0.5 g of KCl was dissolved in 100 g of water and the solution originally at 200 C, froze at 0.240 C.Calculate the percentage dissociation of the salt. (Given :Kf for water = 1.86 K kg /mol, Atomic mass: K = 39 u, Cl= 35.5 u) 40. i) Graphically explain the effect of temperature on the rate cons ...
... (iii) 0.5 g of KCl was dissolved in 100 g of water and the solution originally at 200 C, froze at 0.240 C.Calculate the percentage dissociation of the salt. (Given :Kf for water = 1.86 K kg /mol, Atomic mass: K = 39 u, Cl= 35.5 u) 40. i) Graphically explain the effect of temperature on the rate cons ...
LEGGETT--AP CHEMISTRY * MINIMAL FINAL REVIEW
... and 224 g of NH4Cl, what is the theoretical yield of NH3? (68.1 g). What mass of excess is remaining? (10.3 g) 14. Disulfur dichloride can be made by allowing chlorine gas to react with molten sulfur: S8(l) + 4Cl2(g) 4S2Cl2(g) If you begin with 12.0 g of S8 and 13.03 g Cl2 and you isolate only 15. ...
... and 224 g of NH4Cl, what is the theoretical yield of NH3? (68.1 g). What mass of excess is remaining? (10.3 g) 14. Disulfur dichloride can be made by allowing chlorine gas to react with molten sulfur: S8(l) + 4Cl2(g) 4S2Cl2(g) If you begin with 12.0 g of S8 and 13.03 g Cl2 and you isolate only 15. ...
Chemistry 20 Lesson 36 – The Whole Enchilada
... A portable hydrogen generator uses the reaction of calcium hydride and water to form calcium hydroxide and hydrogen. What volume of hydrogen at 96.5 kPa and 22.0°C can be produce from a 50.0 g cartridge of CaH2 (s)? ...
... A portable hydrogen generator uses the reaction of calcium hydride and water to form calcium hydroxide and hydrogen. What volume of hydrogen at 96.5 kPa and 22.0°C can be produce from a 50.0 g cartridge of CaH2 (s)? ...
Name - Deans Community High School
... b) Is the forward reaction is exothermic or endothermic. ............................................ 1 c) Gold and platinum both catalyse the reaction. For the forward reaction EA using gold is 30 kJ, while EA using platinum is 40 kJ. i) using different dotted lines add this information to the grap ...
... b) Is the forward reaction is exothermic or endothermic. ............................................ 1 c) Gold and platinum both catalyse the reaction. For the forward reaction EA using gold is 30 kJ, while EA using platinum is 40 kJ. i) using different dotted lines add this information to the grap ...
Various Types of RXNS
... --the yellow/orange color of the mixture turns dirty looking, eventually light green (Fe2+) and perhaps to colorless (Fe + Mg2+) 4. 3 H2 + Fe2O3 → 2 Fe + 3 H2O --the iron in the Fe2O3 is reduced to Fe 5. 2 Na + 2 H2O → 2 Na+ + 2 OH- + H2 --if some of the gas is collected in a test tube of air and a ...
... --the yellow/orange color of the mixture turns dirty looking, eventually light green (Fe2+) and perhaps to colorless (Fe + Mg2+) 4. 3 H2 + Fe2O3 → 2 Fe + 3 H2O --the iron in the Fe2O3 is reduced to Fe 5. 2 Na + 2 H2O → 2 Na+ + 2 OH- + H2 --if some of the gas is collected in a test tube of air and a ...
Name: Northwest Vista College Chem 1311
... 44. (6 pts) How many liters of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 with excess HCl(aq) according to the following chemical equation? MnO2(s) + 4HCl(aq) MnCl2(aq) + 2H2O(l) + Cl2(g) Answer: First find the number of moles Cl2 formed from the reaction ...
... 44. (6 pts) How many liters of chlorine gas at 25°C and 0.950 atm can be produced by the reaction of 12.0 g of MnO2 with excess HCl(aq) according to the following chemical equation? MnO2(s) + 4HCl(aq) MnCl2(aq) + 2H2O(l) + Cl2(g) Answer: First find the number of moles Cl2 formed from the reaction ...
Thermodynamics and Kinetics of Solids 21 ________________________________________________________________________________________________________________________
... of isoperibolic or isothermal calorimeters. The substance is being heated to the desired temperature and dropped into the calorimeter. The hot sample is either directly dropped into the liquid within the calorimeter (water, paraffin,...) or into a beaker that is surrounded by water. In the case of p ...
... of isoperibolic or isothermal calorimeters. The substance is being heated to the desired temperature and dropped into the calorimeter. The hot sample is either directly dropped into the liquid within the calorimeter (water, paraffin,...) or into a beaker that is surrounded by water. In the case of p ...
II. Acids and Bases
... 10. For convenience, chemists often use a chemical dye rather than a pH meter to detect the equivalence point of an acid-base titration. 11. Acid-base indicators: chemical dyes whose colors are affected by acidic and basic solutions 12. End point: the point at which the indicator used in a titration ...
... 10. For convenience, chemists often use a chemical dye rather than a pH meter to detect the equivalence point of an acid-base titration. 11. Acid-base indicators: chemical dyes whose colors are affected by acidic and basic solutions 12. End point: the point at which the indicator used in a titration ...
Acid and Bases: Alkalinity and pH in Natural Waters.
... therefore strong acids, e.g., HClO4, HCl, HNO3, and acids that do not have a strong propensity to release protons are therefore weak, e.g. Acetic Acid (Ethanoic: CH3COOH) that we studied in class. The same will hold for bases with respect to their ability to capture protons. It is important to stres ...
... therefore strong acids, e.g., HClO4, HCl, HNO3, and acids that do not have a strong propensity to release protons are therefore weak, e.g. Acetic Acid (Ethanoic: CH3COOH) that we studied in class. The same will hold for bases with respect to their ability to capture protons. It is important to stres ...
1 - Study Hungary
... The pH of an acid solution is 3. It may be a all of the following solutions except. A: 10─3 M HCl solution. B: 10─3 M CH3COOH solution. C: 10─3 M HNO3 solution. D: 10─3 M HBr solution. E: 5 x10─4 M H2SO4 solution. ...
... The pH of an acid solution is 3. It may be a all of the following solutions except. A: 10─3 M HCl solution. B: 10─3 M CH3COOH solution. C: 10─3 M HNO3 solution. D: 10─3 M HBr solution. E: 5 x10─4 M H2SO4 solution. ...
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.