i need full mark on this General chemistry II- 2 quizzes on chapters (11,13,14,15)

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IMPORTANT NOTE for the answers: Results without showing the procedure will not be considered even if the results are correct.

hand-write the results to show the correct procedure. (Always use correct significant figures).

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CHM-112 –General Chemistry II lecture QUIZ # 1 PART A) (only Chapter 11 ) TOT = 50 points Please hand-write your results to show the correct procedure using separate papers. (Always use correct significant figures) Q1_(2pts)_What is the strongest type of intermolecular force present in CHF3? A) ion-dipole B) dispersion C) hydrogen bonding D) dipole-dipole E) None of the above Q2_(2pts)_ What is the strongest type of intermolecular force present in NH2CH3? A) dispersion B) dipole-dipole C) hydrogen bonding D) ion-dipole E) None of the above Q3_(2pts)_What type of intermolecular force causes the dissolution of NaCl in water? A) hydrogen bonding B) dipole-dipole forces C) ion-dipole force D) dispersion forces E) None of the above Q4_ (2pts)_ Choose the molecule or compound that exhibits dispersion forces as its strongest intermolecular force. A) Cl2 B) CO C) HF D) NaCl E) All of these have intermolecular forces stronger than dispersion. Q5_(2pts)_Choose the molecule or compound that exhibits dipole-dipole forces as its strongest intermolecular force. A) H2 B) SO2 C) NH3 D) CF4 E) BCl3 Q6_(2pts)_Choose the compound that exhibits hydrogen bonding as its strongest intermolecular force. A) SCl2 B) C2H6 C) CH3OH D) CH2F2 E) None of the above compounds exhibit hydrogen bonding. Q7_(2pts)_ Place the following compounds in order of increasing strength of intermolecular forces. CO2 F2 NH2CH3 A) NH2CH3 < CO2 < F2 B) F2 < NH2CH3 < CO2 C) NH2CH3 < F2 < CO2 D) F2 < CO2 < NH2CH3 E) CO2 < NH2CH3 < F2 Q8_(2pts)_Place the following compounds in order of increasing strength of intermolecular forces. CH4 CH3CH2CH3 CH3CH3 A) CH3CH2CH3 < CH4 < CH3CH3 B) CH3CH2CH3 < CH3CH3 < CH4 C) CH3CH3 < CH4 < CH3CH2CH3 D) CH4 < CH3CH2CH3 < CH3CH3 E) CH4 < CH3CH3 < CH3CH2CH3 Q9_(2pts)_Place the following compounds in order of decreasing strength of intermolecular forces. HF O2 CO2 A) HF > CO2 > O2 B) HF > O2 > CO2 C) O2 > CO2 > HF D) CO2 > HF > O2 E) CO2 > O2 > HF Q10_(2pts)_Place the following compounds in order of decreasing strength of intermolecular forces. I. CH3CH2CH2CH2CH2CH3 II. (CH3)3CCH3 III. (CH3)3CCH2CH3 A) III > II > I B) I > III > II C) I > II > III D) II > III > I E) III > I > II Q11_(3pts)_Choose the pair of substances that are most likely to form a homogeneous solution. A) NaCl and Hg B) C3H8 and C2H5OH C) LiF and C6H14 D) Br2 and PF3 E) NH3 and CH3OH Q12_(3pts)_Choose the pair of substances that are most likely to form a homogeneous solution. A) C6H14 and C10H20 B) LiBr and C5H12 C) N2O4 and NH4Cl D) C6H14 and H2O E) None of the pairs above will form a homogeneous solution Q13_(3pts)_Choose the substance with the highest surface tension. A) HOCH2CH2OH B) CH2F2 C) CH3CH2F D) CH3CH2OH E) CH3CH2CH3 Q14_(3pts)_Identify the term used to describe the ability of a liquid to flow against gravity up a narrow tube. A) capillary action B) viscosity C) surface tension D) density E) None of the above Q15_(3pts)_Which substance below has the strongest intermolecular forces? A) A2X, ΔHvap = 39.6 kJ/mol B) BY2, ΔHvap = 26.7 kJ/mol C) C3X2, ΔHvap = 36.4 kJ/mol D) DX2, ΔHvap = 23.3 kJ/mol E) EY3, ΔHvap = 21.5 kJ/mol Q16_(3pts)_Place the following substances in order of increasing boiling point. Ne Cl2 O2 A) Ne < Cl2 < O2 B) Cl2 < O2 < Ne C) O2 < Cl2 < Ne D) Cl2 < Ne < O2 E) Ne < O2 < Cl2 Q17_(3pts)_Place the following substances in order of increasing boiling point. CH3CH2OH Ar CH3OCH3 A) Ar < CH3OCH3 < CH3CH2OH B) CH3CH2OH < Ar < CH3OCH3 C) CH3CH2OH < CH3OCH3 < Ar D) CH3OCH3 < Ar < CH3CH2OH E) Ar < CH3CH2OH < CH3OCH3 Q18_(3pts)_Choose the substance with the lowest boiling point. A) H2S B) NBr3 C) F2 D) CF2H2 E) H2O2 Q19_(3pts)_Define sublimation. A) The phase transition from solid to gas. B) The phase transition from gas to solid. C) The phase transition from gas to liquid. D) The phase transition from liquid to gas. E) The phase transition from liquid to solid. Q20_(3pts)_Assign the appropriate labels to the phase diagram shown below. A) A = liquid, B = solid, C = gas, D = critical point B) A = gas, B = solid, C = liquid, D = triple point C) A = gas, B = liquid, C = solid, D = critical point D) A = solid, B = gas, C = liquid, D = supercritical fluid E) A = liquid, B = gas, C = solid, D = triple point QUIZ # 1 PART B (only Chapter13 ) TOT = 50 points Please hand-write your results to show the correct procedure using separate papers. (Always use correct significant figures) Q1_(2pts)_ (Similar as Q4_WORKED_EXAMPLE_1_Chapt12). Lysozyme is an enzyme that cleaves bacterial cell walls. A sample of lysozyme extracted from egg white has a molar mass of 13,930 g. A quantity of 0.100 g of this enzyme is dissolved in 152 g of water at 25°C. Calculate the vapor-pressure lowering, the depression in freezing point, the elevation in boiling point, and the osmotic pressure of this solution. (The vapor pressure of water at 25°C is 23.76 mmHg.). Q2_(2pts)_ ( Similar as Q5_ WORKED_EXAMPLE_1_Chapt12). Two liquids A and B have vapor pressures of 76 mmHg and 132 mmHg, respectively, at 25°C. What is the total vapor pressure of the ideal solution made up of (a) 2.00 mole of A and 3.00 mole of B. Q3_(2pts)_ ( Similar as Q2_WORKED_EXAMPLE_2_Chapt12). What are the boiling point and freezing point of a 2.40 m solution of naphthalene in benzene? (The boiling point and freezing point of benzene are 80.1°C and 5.5°C, respectively.) Q4_ (2pts)_ ( Similar as Q4_WORKED_EXAMPLE_3_Chapt12). A solution is prepared by condensing 5.00 L of a gas, measured at 27°C and 748 mmHg pressure, into 59.0 g of benzene. Calculate the freezing point of this solution. Q5_(2pts)_ (Similar as Q1_WORKED_EXAMPLE_4_Chapt12). What is the osmotic pressure (in atm) of a 1.40 M aqueous solution of urea [(NH2)2CO] at 22.0°C? Q6_(2pts)_ ( Similar as Q4_ PROBLEM_SET_1_Chapt12). What is the molality of a solution formed by dissolving 1.10 mol of KCl in 16.0 mol of water? Q7_(2pts)_ (Similar as Q4_ PROBLEM_SET_1_Chapt12). How many grams of sulfur (S8)must be dissolved in 110.0 g of naphthalene (C10H8) to make a 0.12 m solution? Q8_(2pts)_ EXPLAIN your ANSWER. ( NO EXPLAINATION OR WRONG EXPLAINATION = 0 pts). A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this solution contains 44 ppm chloride ions, the concentration of calcium ions is ________ ppm. Q9_(2pts)_ [ EXPLAIN your ANSWER FOR CASE A) B) C) D) E)]. A 0.100 m solution of which one of the following solutes will have the highest vapor pressure? A) KClO4 B) Ca(ClO4)2 C) Al(ClO4)3 D) sucrose E) NaCl Answer: D Q10_(2pts)_ [ EXPLAIN your ANSWER FOR CASE A) B) C) D) E)]. The magnitudes of Kf and of Kb depend on the identity of the ________. A) solute B) solvent C) solution D) solvent and on temperature E) solute and solvent Answer: B Q11_(3pts)_ [ EXPLAIN your ANSWER FOR CASE A) B) C) D) E) ]. Which of the following liquids will have the lowest freezing point? A) pure H2O B) aqueous glucose (0.60 m) C) aqueous sucrose (0.60 m) D) aqueous FeI3 (0.24 m) E) aqueous KF (0.50 m) Answer: E Q12_(3pts)_ [ EXPLAIN your ANSWER FOR CASE A) B) C) D) E). Which one of the following solutes has a limiting van't Hoff factor (i) of 3 when dissolved in water? A) KNO3 B) CH3OH C) CCl4 D) Na2SO4 E) sucrose Answer: D Q13_(3pts)_ A 2.450.10−2 M solution of NaCl in water is at 20.0∘C. The sample was created by dissolving a sample of NaCl in water and then bringing the volume up to 1.000 L. It was determined that the volume of water needed to do this was 999.3 mL . The density of water at 20.0∘C is 0.9982 g/mL. A) Calculate the molality of the salt solution. Express your answer to four significant figures and include the appropriate units. B) Calculate the mole fraction of salt in this solution. Express the mole fraction to four significant figures. C) Calculate the concentration of the salt solution in percent by mass. Express your answer to four significant figures and include the appropriate units. D) Calculate the concentration of the salt solution in parts per million. Express your answer as an integer to four significant figures and include the appropriate units. Q14_(3pts)_ ( Similar as Q1_ PROBLEM_SET_2_Chapt12). Consider two solutions, one formed by adding 10.00 g of glucose (C6H12O6) to 1 L of water and the other formed by adding 10.00 g of sucrose (C12H22O11) to 1 L of water. Calculate the vapor pressure for each solution at 20 °C; the vapor pressure of pure water at this temperature is 17.50 torr. Q15_(3pts)_ ( Similar as Q10_ PROBLEM_SET_2_Chapt12). Calculate the mass of propylene glycol (C3H8O2) that must be added to 0.34 kg of water to reduce the vapor pressure by 2.880 torr at 40 °C. [Vapor-pressure data for water are –P(H2O) at 40 °C = 55.3 torr] Q16_(3pts)_ ( Similar as Q4_ PROBLEM_SET_2_Chapt12). Using data from your texbook, calculate the freezing and boiling points of each of the following solution: 0.2500 m glucose in ethanol. Q17_(3pts)_ ( Similar as Q5_ PROBLEM_SET_1_Chapt12). A solution is made containing 14.60 g of CH3OH in 184.0 g of H2O. Calculate (a) the mole fraction of CH3OH, (b) the mass percent of CH3OH,(c) the molality of CH3OH Q18_(3pts)_ ( Similar as Q7_ PROBLEM_SET_1_Chapt12). Calculate the molarity of the following aqueous solutions: (a) 0.5400 g of Mg(NO3)2 in 250.00 mL of solution, (b) 22.40 g of LiClO4●3 H2O in 1250 mL of solution, (c) 25.00 mL of 3.500 M HNO3 diluted to 0.2500 L Q19_(3pts)_ ( Similar as Q9_ PROBLEM_SET_1_Chapt12).A sulfuric acid solution containing 571.60 g of H2SO4 per liter of solution has a density of 1.3290 g/cm3. Calculate: (a) the mass percentage, (b) the mole fraction, (c) the molality, (d) the molarity of H 2SO4 in this solution. Q20_(3pts)_ ( Similar as Q2_ PROBLEM_SET_1_Chapt12). (a) What is the mass percentage of iodine in a solution containing 0.0350 mol I2 in 120. g of CCl4? (b) Seawater contains 0.00790 g of Sr2+ per kilogram of water. What is the concentration of Sr2+ in ppm? QUIZ # 1 PART C (only Chapt14) TOT = 50 points Results without showing the procedure will not be considered even if the results are correct. Please hand-write your results to show the correct procedure (you can use separate papers). (Always use correct significant figures). Q1_(2pts)_For the reaction BrO3–+ 5Br–+ 6H+ 3Br2 + 3H2O at a particular time, – [BrO3– ]/ t = 1.5 10–2 M/s. What is – [Br–]/ t at the same instant? A) 13 M/s D) 3.0 10–3 M/s B) 7.5 10–2 M/s E) 330 M/s C) 1.5 10–2 M/s Q2_(2pts)_For the following reaction, P(C6H14)/ t was found to be –6.2 10–3 atm/s. C6H14(g) C6H6(g) + 4H2(g) Determine P(H2)/ t for this reaction at the same time. A) 6.2 10–3 atm/s D) –1.6 10–3 atm/s B) 1.6 10–3 atm/s E) –2.5 10–2 atm/s C) 2.5 10–2 atm/s Q3_(2pts)_For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H2S(g) + O2(g) 2S(s) + 2H2O(l) A) The reaction is third-order overall. B) The reaction is second-order overall. C) The rate law is, rate = k[H2S]2 [O2]. D) The rate law is, rate = k[H2S] [O2]. E) The rate law cannot be determined from the information given. Q4_(2pts)_The reaction A + 2B products has been found to have the rate law, rate = k[A] [B]2. While holding the concentration of A constant, the concentration of B is increased from x to 3x. Predict by what factor the rate of reaction increases. A) 3 B) 6 C) 9 D) 27 E) 30 Q5_(2pts)_The reaction A + 2B products was found to have the rate law, rate = k[A] [B]2. Predict by what factor the rate of reaction will increase when the concentration of A is doubled and the concentration of B is also doubled. A) 2 B) 4 C) 6 D) 8 E) 9 Q6_(2pts)_Appropriate units for a first-order rate constant are A) M/s B) 1/M·s C) 1/s D) 1/M2·s Q7_(2pts)_A rate constant will have the units mol L–1 s–1 when the reaction is overall A) zero order. D) third order. B) first order. E) fourth order. C) second order. Q8_(2pts)_It takes 42.0 min for the concentration of a reactant in a first-order reaction to drop from 0.45 M to 0.32 M at 25°C. How long will it take for the reaction to be 90% complete? A) 13.0 min B) 86.0 min C) 137 min D) 222 min E) 284 min Q9_(2pts)_Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO2(aq) + 2OH–(aq) ClO2–(aq) + ClO3–(aq) + H2O(l) A kinetic study of this reaction under a certain set of conditions yielded the data below. Exp [ClO2] (M) [OH–] (M) 1 2 3 0.0500 0.100 0.100 0.100 0.100 0.0500 - [ClO2] / t (M/s) 5.75 x 10–2 2.30 x 10–1 1.15 x 10–1 Which one of the following is the rate law for this reaction? A) rate = k[ClO2][OH-] D) rate = k[ClO2]2[OH-]2 B) rate = k[ClO2]2[OH-] E) rate = k[ClO2]4[OH-] C) rate = k[ClO2][OH-]2 Q10_(2pts)_The data below were determined for the reaction shown below. S2O82–+ 3I – [S2O82–] [I –] Initial Rate (aq) 2SO42–+ I3–Expt. # 1 0.038 0.060 1.4 10 –5 M/s 2 0.076 0.060 2.8 10 –5 M/s 3 0.076 0.030 1.4 10 –5 M/s Q11_(3pts)_At 25°C the rate constant for the first-order decomposition of a pesticide solution is 6.40 10–3 min–1. If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25°C? A) 1.14 10–1 M D) 2.11 10–2 M B) 47.4 M E) 2.68 10–2 M C) –8.72.0 M Q12_(3pts)_A certain first-order reaction A B is 25% complete in 42 min at 25°C. What is the half-life of the reaction? A) 21 min B) 42 min C) 84 min D) 20 min E) 101 min Q13_(3pts)_A certain first-order reaction A B is 25% complete in 42 min at 25°C. What is its rate constant? A) 6.8 10–3 min–1 D) –3.3 10–2 min–1 B) 8.3 10–3 min–1 E) 11 min–1 C) 3.3 10–2 min–1 Q14_(3pts)_Benzoyl chloride, C6H5COCl, reacts with water to form benzoic acid, C6H5COOH, and hydrochloric acid. This first-order reaction is 25% complete after 26 s. How much longer would one have to wait in order to obtain 99% conversion of benzoyl chloride to benzoic acid? A) 393 s B) 419 s C) 183 s D) 293 s E) 209 s Q15_(3pts)_A certain reaction A products is second order in A. If this reaction is 10.% complete after 20. s, how long would it take for the reaction to be 90.% complete? A) 180 s B) 1600 s C) 440 s D) 18,000 s E) 540 s Q16_(3pts)_For the chemical reaction A B + C, a plot of [A]t versus time is found to give a straight line with a negative slope. What is the order of reaction with respect to A? A) zeroth B) first C) second D) third E) Such a plot cannot reveal the order of the reaction. Q17_(3pts)_The graphs below all refer to the same reaction. What is the order of this reaction? A) zeroth order B) first order C) second order D) unable to predict Q18_(3pts)_What is the slope of an Arrhenius plot for the following reaction? 2NOCl 2NO + Cl2 Temperature k (L/mol·s) (K) 400. 6.6 10–4 500. 2.9 10–1 600. 16.3 A) 8.18 10–2 K B) 5.06 10–2 K C) –1.22 104 K D) –1.96 104 K E) not enough information to calculate the slope Q19_(3pts)_The rate law for the reaction H2O2 + 2H+ + 2I – I2 + 2H2O is rate = k[H2O2][I –]. The following mechanism has been suggested. H2O2 + I – HOI + OH slow – OH –+ H+ H2O HOI + H+ + I – I2 +H2O Fast fast Identify all intermediates included in this mechanism. A) H+ and I –D) H+ only B) H+ and HOI E) H2O and OH– C) HOI and OH– Q20_(3pts)_The following reaction in aqueous solution was found to be first order in [OH–], first order in [C2H5Br], and inverse first order in Br–. C2H5Br + OH– C2H5OH + Br– Which one of the following mechanisms is consistent with the observed reaction order? A) C2H5Br C2H5+ + Br–fast C_2_H_5_+_ _+_ _O_H_–C_2_H_5_O_H_ _slow B) _C_2_H_5_B_r_ _+_H_2_O_ _C_2_H_5_O_H_ _+_ _H_+_ _+_ _B_r_–slow H_+_ _+_ _O_H_–H_2_O C) C2H5Br C2H5+ + Br–slow C_2_H_5_+_ _+_ _O_H_–C_2_H_5_O_H_ _fast D) C2H5Br C2H5+ + Br–slow O_H_–+_ _B_r_–H_O_B_r_ _fast H_O_B_r_ _+_ _C_2_H_5_+_ _C_2_H_5_O_H_ _+_ _B_r_–fast CHEM-112 General Chemistry II lecture QUIZ # 2 PART A (only Chapt15) TOT = 50 points Results without showing the procedure will not be considered even if the results are correct. Please hand-write your results to show the correct procedure (you can use separate papers). (Always use correct significant figures). Q1_(2pts)_Which is the correct equilibrium constant expression for the following reaction? Fe2O3(s) + 3H2(g) 2Fe(s) + 3H2O(g) A) Kc = [Fe2O3] [H2]3 / [Fe]2[H2O]3 D) Kc = [Fe]2[H2O]3 / [Fe2O3] [H2]3 B) Kc = [H2] / [H2O] E) Kc = [Fe] [H2O] / [Fe2O3] [H2] C) Kc = [H2O]3 / [H2]3 Q2_(2pts)_Which of these statements is true about chemical equilibria in general? A) At equilibrium the total concentration of products equals the total concentration of reactants, that is, [products] = [reactants]. B) Equilibrium is the result of the cessation of all chemical change. C) There is only one set of equilibrium concentrations that equals the Kc value. D) At equilibrium, the rate constant of the forward reaction is equal to the rate constant for the reverse reaction. E) At equilibrium, the rate of the forward reaction is equal to as the rate of the reverse reaction. Q3_(2pts)_The following reactions occur at 500 K. Arrange them in order of increasing tendency to proceed to completion (least completion greatest completion). 1) 2NOCl 2NO + Cl2 2) N2O4 2NO2 3) 2SO3 2SO2 + O2 4) 2NO2 2NO + O2 A) 2 < 1 < 3 < 4 B) 3 < 1 < 4 < 2 C) 3 < 4 < 1 < 2 Kp = 1.7 10–2 Kp = 1.5 Kp = 1.3 Kp = 5.9 103 10 –5 10 –5 D) 4 < 3 < 2 < 1 E) 4 < 3 < 1 < 2 Q4_(2pts)_Calculate Kp for the reaction 2NOCl(g) 2NO(g) + Cl2(g) at 400°C if Kc at 400°C for this reaction is 2.1 10–2. A) 2.1 10–2 B) 1.7 10–3 C) 0.70 D) 1.2 E) 3.8 10–4 Q5_(2pts)_On analysis, an equilibrium mixture for the reaction 2H2S(g) 2H2(g) + S2(g) was found to contain 1.0 mol H2S, 4.0 mol H2, and 0.80 mol S2 in a 4.0 L vessel. Calculate the equilibrium constant, Kc, for this reaction. A) 1.6 B) 3.2 C) 12.8 D) 0.64 E) 0.8 Q6_(2pts)_2.50 mol NOCl was placed in a 2.50 L reaction vessel at 400ºC. After equilibrium was established, it was found that 28% of the NOCl had dissociated according to the equation 2NOCl(g) 2NO(g) + Cl2(g). Calculate the equilibrium constant, Kc, for the reaction. A) 0.021 B) 0.039 C) 0.169 D) 26 E) 47 Q7_(2pts)_1.25 moles of NOCl were placed in a 2.50 L reaction chamber at 427ºC. After equilibrium was reached, 1.10 moles of NOCl remained. Calculate the equilibrium constant, Kc, for the reaction 2NOCl(g) 2NO(g) + Cl2(g). A) 3.0 10–4 B) 1.8 103 C) 1.4 10–3 D) 5.6 10–4 E) 4.1 10–3 Q8_(2pts)_The reaction A(g) + 2B(g) C(g) was allowed to come to equilibrium. The initial amounts of reactants placed into a 5.00 L vessel were 1.0 mol A and 1.8 mol B. After the reaction reached equilibrium, 1.0 mol of B was found. Calculate Kc for this reaction. A) 0.060 B) 5.1 C) 17 D) 19 E) 25 Q9_(2pts)_If one starts with pure NO2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g) 2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2. A) 0.152 atm B) 0.174 atm C) 0.200 atm D) 0.326 atm E) The total pressure cannot be calculated because Kp is not given Q10_(2pts)_At 250ºC, the equilibrium constant Kp for the reaction PCl5(g) PCl3(g) + Cl2(g) is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC. Calculate the pressure of PCl5 after the system has reached equilibrium. A) 1.50 atm B) 1.24 atm C) 4.24 atm D) 0.94 atm E) 1.12 atm Q11_(2pts)_Hydrogen iodide decomposes according to the equation 2HI(g) H2(g) + I2(g), for which Kc = 0.0156 at 400ºC. 0.550 mol HI was injected into a 2.00 L reaction vessel at 400ºC. Calculate the concentration of HI at equilibrium. A) 0.138 M B) 0.220 M C) 0.550 M D) 0.275 M E) 0.0275 M Q12_(2pts)_Sodium carbonate, Na2CO3(s), can be prepared by heating sodium bicarbonate, NaHCO3(s). 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) Kp = 0.23 at 100ºC If a sample of NaHCO3 is place ...
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pallveechem123
School: Boston College

quiz 1 is also enclosed

CHM-112 –General Chemistry II lecture
QUIZ # 1 PART A) (only Chapter 11 )TOT = 50 points
Please hand-write your results to show the correct procedure using separate papers.
(Always use correct significant figures)
Q1_(2pts)_What is the strongest type of intermolecular force present in CHF3?
A) ion-dipole
B) dispersion
C) hydrogen bonding
D) dipole-dipole
E) None of the above
Answer:(D) , CH3F has dipole and thus forms dipole -dipole interactions
Q2_ (2pts) _ what is the strongest type of intermolecular force present in NH2CH3?
A) Dispersion
B) dipole-dipole
C) Hydrogen bonding
D) ion-dipole
E) None of the above
Answer: (C) Hydrogen bonding between H attached to NH2 and adjacent molecule N
Q3_ (2pts) _What type of intermolecular force causes the dissolution of NaCl in water?
A) Hydrogen bonding
B) dipole-dipole forces
C) ion-dipole force
D) Dispersion forces
E) None of the above
Answer: (C) NaCl dissolves by forming Na+ and Cl- ions. Thus there is ion - dipole
(water) interactions.
Q4_ (2pts)_ Choose the molecule or compound that exhibits dispersion forces as its
strongest intermolecu...

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