Question paper - Edexcel
... Answer ALL the questions in this section. You should aim to spend no more than 20 minutes on this section. For each question, select one answer from A to D and put a cross in the box . and then mark your new answer with If you change your mind, put a line through the box a cross . 1 Methods for inve ...
... Answer ALL the questions in this section. You should aim to spend no more than 20 minutes on this section. For each question, select one answer from A to D and put a cross in the box . and then mark your new answer with If you change your mind, put a line through the box a cross . 1 Methods for inve ...
Chapter 4
... For acid/base: moles H+ = moles OHUse an indicator to determine endpoint chemical that changes color at endpoint Record volume of second solution 3. Calculate molarity of unknown solution based on molarity and volume of 1 solution and volume recorded in titration. ...
... For acid/base: moles H+ = moles OHUse an indicator to determine endpoint chemical that changes color at endpoint Record volume of second solution 3. Calculate molarity of unknown solution based on molarity and volume of 1 solution and volume recorded in titration. ...
CH1710 PrEX#2 Sp2013 answers
... B) 2 K+(aq) + SO42-(aq) → K2SO4(s) C) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s) D) H22+(aq) + OH-(aq) → H2(OH)2(l) _____ 18. The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution ...
... B) 2 K+(aq) + SO42-(aq) → K2SO4(s) C) H+(aq) + OH-(aq) + 2 K+(aq) + SO42-(aq) → H2O(l) + K2SO4(s) D) H22+(aq) + OH-(aq) → H2(OH)2(l) _____ 18. The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution ...
Exam 3 Review Key
... b) Lead’s primary mode of toxicity is its interference with enzyme function – it mimics other essential metals that take part in enzymatic reactions and displaces them. Considering the fact that sulfhydryl (-SH) groups are found on many enzymes, how might EDTA and DMSA work to treat lead poisoning? ...
... b) Lead’s primary mode of toxicity is its interference with enzyme function – it mimics other essential metals that take part in enzymatic reactions and displaces them. Considering the fact that sulfhydryl (-SH) groups are found on many enzymes, how might EDTA and DMSA work to treat lead poisoning? ...
CHEM102 Chemistry II Spring 10-11 Mid
... A) there is no more chemistry happening. B) the rates of the reaction in the forward and reverse directions are exactly equal. C) the reaction rate in the forward direction is at a maximum. D) the reaction rate in the reverse direction is at a minimum. E) the amounts of reactants and products are ex ...
... A) there is no more chemistry happening. B) the rates of the reaction in the forward and reverse directions are exactly equal. C) the reaction rate in the forward direction is at a maximum. D) the reaction rate in the reverse direction is at a minimum. E) the amounts of reactants and products are ex ...
Masterton and Hurley Chapter 4
... Dye solution that changes color at a set pH Equivalence Point: the place in the titration where the number of moles of acid and moles of base in the flask are equal Endpoint: the place in the titration where the color changes ...
... Dye solution that changes color at a set pH Equivalence Point: the place in the titration where the number of moles of acid and moles of base in the flask are equal Endpoint: the place in the titration where the color changes ...
Ch17-2 Driving Forces of Reactions
... Gas has more entropy than liquid …liquid more entropy than solid S L g Increase in entropy + S …..more crazy random (favored) delta ...
... Gas has more entropy than liquid …liquid more entropy than solid S L g Increase in entropy + S …..more crazy random (favored) delta ...
Name: ______ Date
... a) A process that absorbs energy from its surroundings is called endothermic. b) In an exothermic reaction the enthalpy of species increases. c) Energy is the capacity to do work or to transfer heat. d) Kinetic energy is the energy of motion. There are two properties of a reacting system that determ ...
... a) A process that absorbs energy from its surroundings is called endothermic. b) In an exothermic reaction the enthalpy of species increases. c) Energy is the capacity to do work or to transfer heat. d) Kinetic energy is the energy of motion. There are two properties of a reacting system that determ ...
makeup2
... 61. 2.80 grams of a monoprotic weak acid, HX, was dissolved in water. Titration of the acid to its equivalence point required 29.2 mL of 0.500 M NaOH solution. What is the molecular weight of the acid, HX? (A) 192 g/mol (B) 164 g/mol (C) 96.0 g/mol (D) 5.21 g/mol 62. The ionic reaction 3 I¯ + S2O82¯ ...
... 61. 2.80 grams of a monoprotic weak acid, HX, was dissolved in water. Titration of the acid to its equivalence point required 29.2 mL of 0.500 M NaOH solution. What is the molecular weight of the acid, HX? (A) 192 g/mol (B) 164 g/mol (C) 96.0 g/mol (D) 5.21 g/mol 62. The ionic reaction 3 I¯ + S2O82¯ ...
KEY Final Exam Review - Iowa State University
... a. What is the rate law for the reaction? k[BF3][NH3] seen by exp 1&2;4&5 b. What is the overall order of the reaction? 2 c. Calculate the Rate constant with proper units. Using exp 1 k=(0.2130)M/s/(0.250M)(0.250M)=3.41M-1s-1 could use any of the five to calculate this. kave=3.408M-1s-1 d. What is t ...
... a. What is the rate law for the reaction? k[BF3][NH3] seen by exp 1&2;4&5 b. What is the overall order of the reaction? 2 c. Calculate the Rate constant with proper units. Using exp 1 k=(0.2130)M/s/(0.250M)(0.250M)=3.41M-1s-1 could use any of the five to calculate this. kave=3.408M-1s-1 d. What is t ...
Density of solutions answers The concentration of solutions is often
... What is the enthalpy change for a reaction, and how does this differ from the experimental heat flow measured for an experiment involving the reaction. Use your textbook or a chemical encyclopedia to write a specific definition of the term salt. What does it mean to say that an ion becomes hydrated ...
... What is the enthalpy change for a reaction, and how does this differ from the experimental heat flow measured for an experiment involving the reaction. Use your textbook or a chemical encyclopedia to write a specific definition of the term salt. What does it mean to say that an ion becomes hydrated ...
Document
... Three moles of 1-propanol, C3H7OH, reacts with one mole of phosphorus trichloride to produce 1-chloropropane, C3H7Cl, and phosphorus acid, H3PO3. What is the percent yield if you begin with 75.0 g of both 1propanol and phosphorus trichloride and obtain 1.0 mole of 1-chloropropane? (1propanol= 60.10 ...
... Three moles of 1-propanol, C3H7OH, reacts with one mole of phosphorus trichloride to produce 1-chloropropane, C3H7Cl, and phosphorus acid, H3PO3. What is the percent yield if you begin with 75.0 g of both 1propanol and phosphorus trichloride and obtain 1.0 mole of 1-chloropropane? (1propanol= 60.10 ...
FINAL EXAM Spring 2012
... 10) Determine the pH of the following solution. Initial concentrations are given. [HF] = 1.296 M, [HCl] = 1.045 M, Ka for HF is 6.6 × 10-4 A) -0.019 B) 0.60 C) 1.3 D) 3.1 E) 3.2 11) When 0.10 mol of solid silver nitrate is added to 1.0 L of a clear, saturated solution of Ag2CrO4 (Ksp = 2.4 x 10-12), ...
... 10) Determine the pH of the following solution. Initial concentrations are given. [HF] = 1.296 M, [HCl] = 1.045 M, Ka for HF is 6.6 × 10-4 A) -0.019 B) 0.60 C) 1.3 D) 3.1 E) 3.2 11) When 0.10 mol of solid silver nitrate is added to 1.0 L of a clear, saturated solution of Ag2CrO4 (Ksp = 2.4 x 10-12), ...
Practice Exam #2
... A) The system loses heat and has work done on it by the surroundings. B) The system loses heat and does work on the surroundings. C) The system gains heat and does work on the surroundings. D) The system gains heat and has work done on it by the surroundings. E) None of the above is correct. ...
... A) The system loses heat and has work done on it by the surroundings. B) The system loses heat and does work on the surroundings. C) The system gains heat and does work on the surroundings. D) The system gains heat and has work done on it by the surroundings. E) None of the above is correct. ...
Questions 1-2
... 67. Which of the following describes the changes in forces of attraction that occur as H2O changes phase from a liquid to a vapor? (A) H–O bonds break as H–H and O–O bonds form. (B) Hydrogen bonds between H2O molecules are broken. (C) Covalent bonds between H2O molecules are broken. (D) Ionic bonds ...
... 67. Which of the following describes the changes in forces of attraction that occur as H2O changes phase from a liquid to a vapor? (A) H–O bonds break as H–H and O–O bonds form. (B) Hydrogen bonds between H2O molecules are broken. (C) Covalent bonds between H2O molecules are broken. (D) Ionic bonds ...
Inquiry: Calculation - Coristines
... enthalpy and molar enthalpy. (5 marks) 2. a) Explain the three types of molecular motion as a result of kinetic energy (3marks) b) Why does neon have a lower molar heat capacity than nitrogen ? (2 mark) C) When a fire extinguisher is filled the container becomes very warm and when it is discharged t ...
... enthalpy and molar enthalpy. (5 marks) 2. a) Explain the three types of molecular motion as a result of kinetic energy (3marks) b) Why does neon have a lower molar heat capacity than nitrogen ? (2 mark) C) When a fire extinguisher is filled the container becomes very warm and when it is discharged t ...
Sample
... 48- Which of the following reactions represents an increasing in entropy? a) Formation of crystals from solution b) Formation of one mole of gas from two moles of reactant gases c) Dissolving of crystals in a solution d) Condensation of water vapor into liquid water. 49- Under which of the following ...
... 48- Which of the following reactions represents an increasing in entropy? a) Formation of crystals from solution b) Formation of one mole of gas from two moles of reactant gases c) Dissolving of crystals in a solution d) Condensation of water vapor into liquid water. 49- Under which of the following ...
Chapter 3
... Trade partners – A goes with D and C goes with B. Once again, charges MUST be observed when recombining and formulas are written with cation first. Reaction only happens if one of the two products is Insoluble (s). LEP #14 a, b ...
... Trade partners – A goes with D and C goes with B. Once again, charges MUST be observed when recombining and formulas are written with cation first. Reaction only happens if one of the two products is Insoluble (s). LEP #14 a, b ...
Exam 2 Fall 2005 Chemsitry 1211
... a.) H+ (aq) + F- (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + 2H+ (l) + O-2 (l) b) H+ (aq) + F- (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + H2O (aq) c.) HF (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + H2O(l) d.) HF (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + 2H+ (l) + O-2 (l) e.) HF (a ...
... a.) H+ (aq) + F- (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + 2H+ (l) + O-2 (l) b) H+ (aq) + F- (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + H2O (aq) c.) HF (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + H2O(l) d.) HF (aq) + K+ (aq) + OH- (aq) K+ (aq) + F- (aq) + 2H+ (l) + O-2 (l) e.) HF (a ...
Chemistry Spring Final Review
... 47. Predict the product, balance the equation, and choose the correct coefficient for the underlined compound. Ethane (C2H6) combusts A. 6 B. 2 C. 3 D. 1 48. Predict the product, balance the equation, and choose the correct coefficient for the underlined compound. Manganese (VI) oxide reacts with c ...
... 47. Predict the product, balance the equation, and choose the correct coefficient for the underlined compound. Ethane (C2H6) combusts A. 6 B. 2 C. 3 D. 1 48. Predict the product, balance the equation, and choose the correct coefficient for the underlined compound. Manganese (VI) oxide reacts with c ...
chemistry 102 fall 2001 part 1
... (2) Each multiple choice question is actually 2 questions on your scanning sheet. If you are sure of an answer, put the same answer down for both questions for 5 pts. If you cannot decide between two answers, put one answer down for one question and the other answer down for the other question. If y ...
... (2) Each multiple choice question is actually 2 questions on your scanning sheet. If you are sure of an answer, put the same answer down for both questions for 5 pts. If you cannot decide between two answers, put one answer down for one question and the other answer down for the other question. If y ...
Chemistry Final Exam Test Yourself I
... (g), the equilibrium constant at a particular temperature is 0.050. The concentrations of each substance are the following: [N2] = 0.5 M, [O2] = 1.7 M, [NO] = 0.010 M. Which way will the reaction shift so as to achieve equilibrium? (Q = 1 x 10-4 Reaction will shift to the right) ...
... (g), the equilibrium constant at a particular temperature is 0.050. The concentrations of each substance are the following: [N2] = 0.5 M, [O2] = 1.7 M, [NO] = 0.010 M. Which way will the reaction shift so as to achieve equilibrium? (Q = 1 x 10-4 Reaction will shift to the right) ...
Pages from PS 11 Textbook for Lab
... where qp is the heat released at constant pressure. This new state variable, H, is called the enthalpy and ∆H = qp is the enthalpy change for a chemical process at constant pressure, which is the thermal energy (heat) produced by the chemical reaction at constant pressure. Because we live, by and la ...
... where qp is the heat released at constant pressure. This new state variable, H, is called the enthalpy and ∆H = qp is the enthalpy change for a chemical process at constant pressure, which is the thermal energy (heat) produced by the chemical reaction at constant pressure. Because we live, by and la ...
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.