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Ethers have... o higher than expected boiling point o low boiling points hydrogen bond towards eachother...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding. The...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding. The structure of 3-methylbutyric acid is shown below. Draw a second molecule of 3-methylbutyric acid - oriented in the most stable dimeric configuration with the other molecule of acid-and show the intermolecular hydrogen bonds. To indicate a hydrogen bond, draw a regular single bond between the atoms, then click on the "graded select" tool (the yellow highlighter) and click on the bond. A selected bond...
C The boiling point of H,O is much higher than the boiling point of HS. H2O...
C The boiling point of H,O is much higher than the boiling point of HS. H2O is a molecular compound, while HS is an ionic compound. H2O is a polar molecule, so the attractions between the molecules are stronger than those between nonpolar H2S molecules. H2O has strong hydrogen bonds between its molecules, and HS molecules cannot form hydrogen bonds. The dispersion forces between the H2O molecules are much stronger. d The boiling point of CH,O is much higher than...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding. Several...
Carboxylic acids have higher than expected boiling points due to
dimeric associations involving hydrogen bonding. Several dimers of
3‑methylbutanoic acid (3‑methylbutyric acid) are shown where
proposed hydrogen bonding is represented by a dotted line.
Select the pair of compounds that show all of the expected
hydrogen bonds in a carboxylic acid dimer.
CH C HzCº. ---- H_CH, T 0 O= CH3 IM CH3 CH3 0 CH3 CH lyon НС 0- To CH3 IO-o CH3 Ó CH3 LCH C. Hzc OH...
Part A H,0 (100°C) has a higher boiling point than CH, OH (65°C). There are more...
Part A H,0 (100°C) has a higher boiling point than CH, OH (65°C). There are more hydrogen bonds between water molecules than between alcohol molecules. There are less hydrogen bonds between water molecules than between alcohol molecules. CH, OH has the higher molecular mass than H,O. There are no hydrogen bonds between alcohol molecules while there are plenty of them between water molecules. O Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining Part B H,O (100°C)...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding, Several...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding, Several dimers of 3-methylbutanoic acid (3-methylbutyric acid) are shown where proposed hydrogen bonding is represented by a dotted line. Select the pair of compounds that show all of the expected hydrogen bonds in a carboxylic acid dimer. CH3 0 HC 90 H3C CH3 0 CH HyComo сно < Assignment Score: 9.5% Resources < Question 11 of 20 > Io H3C H3C HCH₂ =0 HEC H...
47. Which is expected to have a higher boiling point, C&H18 or CaH1o? A) C3H18 B)...
47. Which is expected to have a higher boiling point, C&H18 or CaH1o? A) C3H18 B) САН1о all of the above C) none of the above D
2 Why is the boiling point of ammonia higher than the boiling point of ethane? What...
2 Why is the boiling point of ammonia higher than the boiling point of ethane? What type of interaction is responsible for sodium chloride's very high melting point? A 5. What type of interaction is responsible for water's high boiling point? 4 A gaseous sample of a compound has a gas density of 0.647 g/L at 694 torr and 20 °C. What is the molar mass of this compound? If this compound contains only nitrogen and hydrogen, and is 82.2%...
-give reasone SH bond is less polar than OH bond. Hydrogen bonding is much weakerin thiols...
-give reasone SH bond is less polar than OH bond. Hydrogen bonding is much weakerin thiols than in alcohols. 2. Thiols are less soluble in water than alcohols. Thiols have low boiling points than alcohols
Question 14 1 pts Why is the boiling point of an aqueous solution higher than the...
Question 14 1 pts Why is the boiling point of an aqueous solution higher than the boiling point of pure water? Because the temperature increases Because the liquid/gas equilibrium slope is positive on the phase diagram Because the total pressure decreases due to the solute o Because the vapor pressure decreases due to the solute None of the options explain why the boiling point increases
Alcohols have melting and boiling points higher than most other compounds of similar molar mass due...
Alcohols have melting and boiling points higher than most other compounds of similar molar mass due to D A lonic bonds OB dipol-dipole interactions OC London dispersion forces OD hydrogen bonds
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding. The structure of 3-methylbutyric acid is shown below. Draw a second molecule of 3-methylbutyric acid - oriented in the most stable dimeric configuration with the other molecule of acid-and show the intermolecular hydrogen bonds. To indicate a hydrogen bond, draw a regular single bond between the atoms, then click on the "graded select" tool (the yellow highlighter) and click on the bond. A selected bond...
C The boiling point of H,O is much higher than the boiling point of HS. H2O is a molecular compound, while HS is an ionic compound. H2O is a polar molecule, so the attractions between the molecules are stronger than those between nonpolar H2S molecules. H2O has strong hydrogen bonds between its molecules, and HS molecules cannot form hydrogen bonds. The dispersion forces between the H2O molecules are much stronger. d The boiling point of CH,O is much higher than...
Carboxylic acids have higher than expected boiling points due to
dimeric associations involving hydrogen bonding. Several dimers of
3‑methylbutanoic acid (3‑methylbutyric acid) are shown where
proposed hydrogen bonding is represented by a dotted line.
Select the pair of compounds that show all of the expected
hydrogen bonds in a carboxylic acid dimer.
CH C HzCº. ---- H_CH, T 0 O= CH3 IM CH3 CH3 0 CH3 CH lyon НС 0- To CH3 IO-o CH3 Ó CH3 LCH C. Hzc OH...
Part A H,0 (100°C) has a higher boiling point than CH, OH (65°C). There are more hydrogen bonds between water molecules than between alcohol molecules. There are less hydrogen bonds between water molecules than between alcohol molecules. CH, OH has the higher molecular mass than H,O. There are no hydrogen bonds between alcohol molecules while there are plenty of them between water molecules. O Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining Part B H,O (100°C)...
Carboxylic acids have higher than expected boiling points due to dimeric associations involving hydrogen bonding, Several dimers of 3-methylbutanoic acid (3-methylbutyric acid) are shown where proposed hydrogen bonding is represented by a dotted line. Select the pair of compounds that show all of the expected hydrogen bonds in a carboxylic acid dimer. CH3 0 HC 90 H3C CH3 0 CH HyComo сно < Assignment Score: 9.5% Resources < Question 11 of 20 > Io H3C H3C HCH₂ =0 HEC H...
47. Which is expected to have a higher boiling point, C&H18 or CaH1o? A) C3H18 B) САН1о all of the above C) none of the above D
2 Why is the boiling point of ammonia higher than the boiling point of ethane? What type of interaction is responsible for sodium chloride's very high melting point? A 5. What type of interaction is responsible for water's high boiling point? 4 A gaseous sample of a compound has a gas density of 0.647 g/L at 694 torr and 20 °C. What is the molar mass of this compound? If this compound contains only nitrogen and hydrogen, and is 82.2%...
-give reasone SH bond is less polar than OH bond. Hydrogen bonding is much weakerin thiols than in alcohols. 2. Thiols are less soluble in water than alcohols. Thiols have low boiling points than alcohols
Question 14 1 pts Why is the boiling point of an aqueous solution higher than the boiling point of pure water? Because the temperature increases Because the liquid/gas equilibrium slope is positive on the phase diagram Because the total pressure decreases due to the solute o Because the vapor pressure decreases due to the solute None of the options explain why the boiling point increases
Alcohols have melting and boiling points higher than most other compounds of similar molar mass due to D A lonic bonds OB dipol-dipole interactions OC London dispersion forces OD hydrogen bonds
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