18. ( \( \mathbf{1 0} \) points) The table below shows the normal boiling points of some compounds containing \( \mathrm{C}=\mathrm{O} \) groups. \begin{tabular}{|c|c|c|} \hline Compound & Structure & Normal boiling point ( \( { }^{\circ} \mathrm{C} \) ) \\ \hline \( \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O} \) (ethanal) & & 20.2 \\ \hline \( \mathrm{CH}_{2} \mathrm{O}_{2} \) (methanoic acid) & & 100.8 \\ \hline \( \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}_{2} \) (ethanoic acid) & & 118.1 \\ \hline \( \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{2} \) (methyl ethanoate) & & 56.9 \\ \hline \end{tabular} (a) Which of these compounds exhibit dispersion forces? (b) Which of these compounds exhibit dipole-dipole forces? (c) Which of these compounds exhibit hydrogen bonding? (d) Why is the boiling point of ethanoic acid higher than that of methanoic acid? (e) Why is the boiling point of ethanal the lowest of all?
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- Dispersion forces (London forces) are present in all molecules. - Dipole-dipole forces occur in polar molecules. - Hydrogen bonding occurs in molecules with N-H, O-H, or F-H bonds. Show more…
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The table below shows the normal boiling points of some compounds containing $\mathrm{C}=\mathrm{O}$ groups. (a) Which of these compounds exhibit dispersion interactions? (b) Which of these compounds exhibit dipole-dipole interactions? (c) Which of these compounds exhibit hydrogen bonding? (d) Why is the boiling point of ethanoic acid higher than that of methanoic acid? (e) Why is the boiling point of ethanal the lowest of all?
b.) Draw a circle around each polar or nonpolar region of the carbon compounds below, and LABEL EACH REGION with the TYPE of INTERMOLECULAR ATTRACTIVE FORCE that it could use to interact with neighboring molecules of the same kind. c.) Predict the relative boiling points of the five compounds by ranking them #1 through #5 (with #1 = HIGHEST boiling point temperature, #5 = LOWEST boiling point temperature). Indicate each compound with its chemical formula. (HIGHEST) #1 = ________#2 = ________#3 = ________#4 = ________#5 = ________ (LOWEST) d.) Briefly explain your reasoning for the compounds you selected with the highest and lowest boiling point temperatures. e.) For the highest boiling point substance – draw a Lewis structure sketch to illustrate the attractive forces between several (at least three) molecules of this compound. 2. The ideal gas law describes the behavior of substances in the vapor phase. You will determine the pressure (P), volume (V), and temperature (T) of a fixed number of moles of hydrogen gas (n), produced by reacting magnesium metal with hydrochloric acid: Mg (s) + 2 HCl (aq) → H2 (g) + MgCl2 (aq) Determine the number of moles of hydrogen gas formed when a 4.5 mm length of Mg ribbon reacts with excess hydrochloric acid (HCl). You will need a molar mass (from the Periodic Table), the mole relationship from the balanced chemical equation, and the unit relationship: 1.00 meter of Mg ribbon = 0.500 grams.
Sri K.
Compute the determinant using a cofactor expansion across the first row. Also compute the determinant by a cofactor expansion down the second column. Write the expression for the determinant using a cofactor expansion across the first row. Choose the correct answer below. Using this expansion, the determinant is (7)(55)-(-7)(71)+(8)(65). Using this expansion, the determinant is (7)(-57)+(-7)(-15)+(8)(63). Write the expression for the determinant using a cofactor expansion down the second column. Choose the correct answer below. Using this expansion, the determinant is (-7)(-15)+(1)(-15)+(8)(-15). Using this expansion, the determinant is (-7)(-15)+(1)(-15)-(8)(-15). The determinant is (Simplify your answer).
Adi S.
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