10. Which intermolecular interaction is predominant between ethylacetate (CH3COOCH₂CH3) and ethanol (CH3CH₂OH)? A. dipole-induced dipole B. dipole-dipole X C. dispersion D. hydrogen bond E. ion-dipole X polar molecule FN₂O
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- Use molecular structures and noncovalent interactions to explain why dimethyl ether, (CH3)2O, is completely miscible in water, but dimethylsulfide, (CH3)2S, is only slightly water soluble.Consider the data in the table. Compound Melting point (°C) ????? (??/???)ΔHfus (kJ/mol) Boiling point (°C) ????? (??/???)ΔHvap (kJ/mol) HFHF −83.11 4.577 19.54 25.18 HClHCl −114.3 1.991 −84.9 17.53 HBrHBr −86.96 2.406 −67.0 19.27 HIHI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ?fusΔSfus and Δ?vapΔSvap for HF.HF. Δ?fus=ΔSfus= J/(K⋅mol)J/(K⋅mol) Δ?vap=ΔSvap= J/(K⋅mol)J/(K⋅mol) Determine the entropy change when 7.60 mol HF(l)7.60 mol HF(l) boils at atmospheric pressure. Δ?=ΔS= J/KConsider the data in the table. Compound Melting point (°C) ????? (??/???)ΔHfus (kJ/mol) Boiling point (°C) ????? (??/???)ΔHvap (kJ/mol) HFHF −83.11 4.577 19.54 25.18 HClHCl −114.3 1.991 −84.9 17.53 HBrHBr −86.96 2.406 −67.0 19.27 HIHI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ?fus and Δ?vap for HF. Δ?fus= J/(K⋅mol) Δ?vap= J/(K⋅mol) Determine the entropy change when 8.70 mol HF(g) condenses at atmospheric pressure. Δ?= J/K
- In comparing the reactants to the products, in the reaction below, what layer of a separation funnel would the REACTANTS bind to and why? H3C. CH, CH3 он HC. CH: CH2 но CH2 A) The hydrophillic layer, the H-bonding groups B) The hydrophobic layer, the H-bonding groups C) the hydrophillic layer, the dispersion forces with a single dipole shielded by methyl groups D) the hydrophobic layer, the dispersion forces with a single dipole shielded by methyl groups7. Which of the following would behave as a hydrogen bond acceptor, but not a hydrogen bond donor? H H:0: H I || | Н-с-с-с-н H :0: H ннн ннн Н-с-с-с—Н Н-с-с-с-о- Н-с-с-с-N-H ннн H ннн ннннWhat main type of forces must be disrupted between CH3OH molecules when Br2 dissolves? hydrogen bonding dipole-dipole dipole-induced dipole induced dipole-induced dipole
- What is the dominant IMF in the molecule CH3CHCHCOOH? A.dispersion forces B. Dipole-dipole C. Hydrogen bonding D. Ion-ion12. Normal boiling point of ethanol (C2H5OH) is 78 °C, and of propanol (C3H;OH) is 97 °C. a. Explain the reason for the difference in boiling points of these two alcohols. b. When the underline methyl group in propanol, CH3CH2CH2OH, is replaced with a hydroxyl group (HOCH2CH2OH), boiling point of the molecule increases to 197 °C. Explain the reason for observed increase in the boiling point.1) CI (1 equiv) cat. AICI3 2) HNO3, cat. H2SO4 CI
- Which of the following compounds has the lowest boiling point? 2 He H 10 thim bem temn megin] 10 Li Be C N F Ne monphone 15 arge 11 12 13 14 16 17 18 Na Mg AI Si ci Ar 26 tromine 35 19 20 21 22 23 24 25 27 28 29 30 31 32 33 34 к Са Sc Ti vCr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr etem 41 theum p m 46 ede 37 38 39 40 42 43 44 45 47 48 49 50 52 53 54 Rb Sr Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Хе 112 bert hath than hemth abe 55 56 57-70 71 72 73 74 75 76 77 70 79 82 83 85 Cs Ba Lu Hf Ta w Re Os Ir Pt Au Hg TI Pb Bi Po At Rn 87 85-102 103 104 105 106 107 108 100 110 111 112 114 Fr Ra ** Lr Rf Db Sg Bh Hs Mt Uun Uuu Uub Uuq 223 61 65 67 70 *Lanthanide series La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb 174 **Actinide series 91 92 93 94 95 96 97 99 100 101 102 Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No pe pe Select one: O a. CH;CH2CH;CH2OH O b. C(CH3)4 Oc CH3CH2CH2CH2F d. (CH;);COH O e. CH;CH2CH;CH2CH3Aspirin has a higher molar mass compared to salicylic acid, however aspirin melts at a lower temperature than salicylic acid. Provide a brief explanation for this observation. Table 1 Compound: Formula: Salicylic Acid C;H6O3 Aspirin C9H3O4 Molar Mass: 138.12 Melting point: Ka 158-160°C 1.08 x 10³ 180.15 140-142°C 2.72 x 10$ pKa Solubility (g/100ML) 2.99 4.57 0.18 0.2510B5. Answer both parts to this question.