Terms in this set (12)Based only on intermolecular forces, which of the following would be the least soluble in CH₃CH₂OH CH₃CH₃ Molecules with a C-O or O-H bond can experience both dipole-dipole and hydrogen bonding interaction with CH₃CH₂OH, while CH₃CH₃ can only experience dispersion forces, so CH₃CH₃ will be the least soluble in CH₃CH₂OH. C₆H₁₄ is soluble in C₅H₁₂. In H₂O, this solute would be Less soluble Dispersion forces vary with the size of the molecule, so they would be stronger between C₆H₁₄ and C₅H₁₂ than between C₆H₁₄ and H₂O. Furthemore C₆H₁₄ in H₂O interrupts the strong hydrogen bonding between H₂O molecules, so C₆H₁₄ is less soluble in H₂O than in C₅H₁₂. What intermolecular forces are shared between CH₃CH₂CH₂F and CH₃CH₂CH₂OH? Dispersion forces and dipole-dipole forces Both molecules (as do all molecules) experience dispersion forces, and both have polar bonds (C-F in one case, C-O in the other). Only CH₃CH₂CH₂OH has the feature which can exhibit hydrogen bonding, a hydrogen atom attached to a highly electronegative atom such as O What intermolecular forces are shared between CH₃F and CF₄? Dispersion forces only Both molecules (as do all molecules) experience dispersion forces. While CF₄ has polar C-F bonds, they are symmetrically located and there is no net dipole in the molecule, and therefore no dipole-dipole force. Neither molecule has the feature which which can exhibit hydrogen bonding, a hydrogen atom attached to a highly electronegative atom such as F, O or N. Based only on intermolecular forces, which of the following pairs of molecules would be expected to form an endothermic solution? CH₃CH₂CH₂OCH₃ and CH₃CH₂CH₂CH₂OH For a solution to be endothermic, either the solute-solute or solvent-solvent attractions must be stronger than the solute-solvent attractions. This will be the case for C) CH₃CH₂CH₂OCH₃ and CH₃CH₂CH₂CH₂OH, where the hydrogen bonding between CH₃CH₂CH₂CH₂OH molecules will be stronger than the solute-solvent attractons. Choice B) CH₃CH₂CH₂CH₂CH₃ and CH₃CH₂CH₂CH₃ should be close to ideal, and choices A and B should be immiscible and not form a solution. Based only on their intermolecular forces, which of the following pairs of molecules would be soluble in one another? CH₃CH₂CH₂OCH₃ and CH₃CH₂CH₂CH₂OH Substances with similar intermolecular attractive forces tend to be soluble in one another. Only CH₃CH₂CH₂OCH₃ and CH₃CH₂CH₂CH₂OH both have dipole-dipole interactions and would be soluble in one another. The other pairs all consist of one polar and one nonpolar compound. Which of the following would become more soluble in water at higher pressure? N₂ (g) Changes in pressure only affect solutions containing a gaseous solute. Henry's Law states that the higher the partial pressure of the gas, the more soluble it will be in the solvent. This is because there are more molecules of the solute available to dissolve in the solvent. Also, gases generally become less soluble at higher temperatures because there is more kinetic energy in the system, and the gas molecules are more likely to have enough energy to leave the solvent. Which of the following would become more soluble in water at lower temperature? O₂ (g) Gases generally become more soluble at lower temperatures because there is less kinetic energy in the system, and the gas molecules are less likely to have enough energy to leave the solvent. Which of the following aqueous solutions would have the highest boiling point? 1.0 m CaCl₂ The dissolved solute will raise the boiling point. The more "things" that are dissolved (ions or molecules), the higher the boiling point will be. The CaCl₂ will break up into one Ca²⁺ ion and two Cl⁻ ions and there will be a concentration of 3.0 m of "things" in solution. The other choices will have fewer "things" in solution and will raise the boiling point less. Which one of the following aqueous solutions would have the highest freezing point? 1.0 m C₆H₁₂O₆ The dissolved solute will lower the freezing point. The more "things" that are dissolved (ions or molecules), the lower the freezing point will be. Since C₆H₁₂O₆ is a molecule, it will not break apart and there will only be a concentration of 1.0 m of molecules in solution. It will lower the freezing point less than all the other choices. There will be fewer "things" in solution and this will lower the freezing point less than the other choices Which of the following solutes will lower the freezing point the most in 1 L H₂O? 1 mol MgI₂ All of these compounds are soluble in water so they will all break up into ions. The more ions there are in solution, the bigger the change to the freezing point (and boiling point). Since MgI₂ will break up into one magnesium ion and two iodide ions, it will produce more ions in solution than the other two choices.c Which of the following ions will contribute most to elevating the boiling point of H₂O? ... 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The solid-liquid boundary is given by $p / bar =p_{3} / bar + 1000(5.60+11.727 x) x$ where $x=T / T_{3}-1$ and the triple point pressure and temperature are $p_{3}= 0.4362\ \mu b a r$ and $T_{3}=178.15\ \mathrm{K}.$ The liquid-vapour curve is given by $\ln (p / bar) = -10.418 / y+ 21.157-15.996 y + 14.015 y^{2} - 5.0120 y^{3} + 4.7334(1-y)^{1.70}$ where $y=T / T_{e}=T /(593.95\ K).$ (a) Plot the solid-liquid and liquid-vapour phase boundaries. (b) Estimate the standard melting point of methylbenzene. (c) Estimate the standard boiling point of methylbenzene. (The equation you will need to solve to find this quantity cannot be solved by hand, so you should use a numerical approach, e.g. by using mathematical software.) (d) Calculate the standard enthalpy of vaporization of methylbenzene at the standard boiling point, given that the molar volumes of the liquid and vapour at the standard boiling point are $0.12\ \mathrm{dm}^{3}\ \mathrm{mol}^{-1}$ and $30.3\ \mathrm{dm}^{3}\ \mathrm{mol}^{-1},$ respectively. Verified answer
chemistry Carry out each of the following calculations, paying special attention to significant figures, rounding, and units (J = joule, the Sl unit of energy; mol = mole, the SI unit for amount of substance): (a) $\frac { \left( 6.626 \times 10 ^ { - 34 } \mathrm { J } \cdot \mathrm { s } \right) \left( 2.9979 \times 10 ^ { 8 } \mathrm { m } / \mathrm { s } \right) } { 489 \times 10 ^ { - 9 } \mathrm { m } }$, (b) $\frac { \left( 6.022 \times 10 ^ { 23 } \text { molecules/mol } \left( 1.23 \times 10 ^ { 2 } \mathrm { g } \right) \right. } { 46.07 \mathrm { g } / \mathrm { mol } }$, (c) $\left( 6.022 \times 10 ^ { 23 } \text { atoms } / \operatorname { mol } \right) \left( 2.18 \times 10 ^ { - 18 } \text { J/atom) } \left( \frac { 1 } { 2 ^ { 2 } } - \frac { 1 } { 3 ^ { 2 } } \right)\right.$ where the number 2 and 3 in the last term are exact. Verified answer chemistry It is common to make measurements of absorbance at two wavelengths and use them to find the individual concentrations of two components A and B in a mixture Show that the molar concentrations of A and B in a cell of length L are $[\mathbf{A}]=\frac {\epsilon_{{B2}}A_1- \epsilon_{{B1}}A_2}{(\epsilon_{{A1}}\epsilon_{{B2}}-\epsilon_{{A2}}\epsilon_{{B1}})L}$ $[\mathbf{B}]=\frac {\epsilon_{{A2}}A_2- \epsilon_{{A1}}A_1}{(\epsilon_{{A1}}\epsilon_{{B2}}-\epsilon_{{A2}}\epsilon_{{B1}})L}$ where $A_{1}$ and $A_{2}$ are absorbances of the mixture at wavelengths $\lambda_{1}$ and $\lambda_{2}$ the molar extinction coefficients of A (and B) at these wavelengths are $\epsilon_{{A1}}$ and $\epsilon_{{A2}}$ (and $\epsilon_{{B1}}$ and $\epsilon_{{B2}})$. Verified answer Recommended textbook solutions Organic Chemistry3rd EditionDavid Klein 3,028 solutions Quantitative Chemical Analysis8th EditionDaniel C. Harris 921 solutions Principles of Environmental Chemistry3rd EditionJames Girard 371 solutions
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Based only on intermolecular forces, which of the following would be the least soluble in ch₃ch₂oh?
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