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Chapter 9: Problem 68

In the blanks provided, answer the questions below, using LT (for is less than), GT (for is greater than), \(\mathrm{EQ}\) (for is equal to), or MI (for more information required). (a) The boiling point of \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(\mathrm{MM}=60.0 \mathrm{~g} / \mathrm{mol})\) the boiling point of \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{C}=\mathrm{O}(\mathrm{MM}=58.0 \mathrm{~g} / \mathrm{mol})\). (b) The vapor pressure of \(\mathrm{X}\) is \(250 \mathrm{~mm} \mathrm{Hg}\) at \(57^{\circ} \mathrm{C}\). Given a sealed flask at \(57^{\circ} \mathrm{C}\) that contains only gas, the pressure in the flask \(245 \mathrm{~mm} \mathrm{Hg}\) (c) The melting-point curve for Y tilts to the right of a straight line. The density of \(\mathrm{Y}(l) \quad\) the density of \(\mathrm{Y}(s)\). (d) The normal boiling point of \(\mathrm{A}\) is \(85^{\circ} \mathrm{C}\), while the normal boiling point of \(\mathrm{B}\) is \(45^{\circ} \mathrm{C}\). The vapor pressure of \(\mathrm{A}\) at \(85^{\circ} \mathrm{C}\) pressure of \(\mathrm{B}\) at \(45^{\circ} \mathrm{C}\). (e) The triple point of \(A\) is \(25 \mathrm{~mm} \mathrm{Hg}\) and \(5^{\circ} \mathrm{C}\). The melting point of \(\mathrm{A}\) \(5^{\circ} \mathrm{C}\)

Short Answer

Expert verified
Question: Compare the following properties of given substances using the relationships LT (less than), GT (greater than), EQ (equal), or MI (more information required): (a) Boiling point of a compound with a molar mass of 150 g/mol ______ boiling point of a compound with a molar mass of 190 g/mol. (b) Vapor pressure of substance X at 57°C (250 mm Hg) ______ total pressure in a flask containing only gas at 57°C (245 mm Hg). (c) Density of substance Y in the liquid state ______ density of Y in the solid state, given that the melting-point curve for Y tilts to the right of a straight line. (d) Vapor pressure of substance A at its normal boiling point (125°C) ______ vapor pressure of substance B at its normal boiling point (90°C). (e) Melting point of substance A (5°C) ______ temperature at the triple point of A (25 mm Hg, 5°C). Answer: (a) MI (b) GT (c) LT (d) EQ (e) EQ

Step by step solution

01

(a) Boiling Point Comparison

In question (a), we are given the molar mass of two compounds, and we need to compare their boiling points. However, without knowing their chemical properties and boiling point trends, we cannot infer the comparison of their boiling points. So, the correct answer for (a) is MI (more information required).
02

(b) Vapor Pressure Comparison

In question (b), we are given the vapor pressure of substance X at 57°C and the total pressure in a flask that contains only gas at the same temperature. Since the vapor pressure of the substance X is 250 mm Hg and the total pressure in the flask is 245 mm Hg, we can infer that the pressure of X is GT (greater than) the pressure in the flask.
03

(c) Density Comparison

In question (c), we are given the melting-point curve for substance Y tilts to the right of a straight line. This implies that the substance is expanding as it melts. Therefore, the density of Y in the liquid state is LT (less than) the density of Y in the solid state.
04

(d) Vapor Pressure Comparison

In question (d), we are given the normal boiling points of substances A and B and asked to compare their vapor pressures at these points. At the normal boiling point, the vapor pressure of a substance is equal to 1 atmosphere (760 mm Hg). Since both substances are at their respective boiling points, their vapor pressures are EQ (equal) at these temperatures.
05

(e) Melting Point Comparison

In question (e), we are given that the triple point of A is at 25 mm Hg and 5°C. The melting point of A is also given as 5°C. At the triple point, all three phases of a substance coexist. Since the melting point and the temperature of the triple point are the same, we can conclude that the melting point of A is EQ (equal) to the temperature at the triple point, which is 5°C.

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Most popular questions from this chapter

The density of liquid mercury at \(20^{\circ} \mathrm{C}\) is \(13.6 \mathrm{~g} / \mathrm{cm}^{3}\), its vapor pressure is \(1.2 \times 10^{-3} \mathrm{~mm} \mathrm{Hg}\). (a) What volume (in \(\mathrm{cm}^{3}\) ) is occupied by one mole of \(\mathrm{Hg}(l)\) at \(20^{\circ} \mathrm{C}\) ? (b) What volume (in \(\mathrm{cm}^{3}\) ) is occupied by one mole of \(\mathrm{Hg}(\mathrm{g})\) at \(20^{\circ} \mathrm{C}\) and the equilibrium vapor pressure? (c) The atomic radius of \(\mathrm{Hg}\) is \(0.155 \mathrm{~nm}\). Calculate the volume (in \(\mathrm{cm}^{3}\) ) of one mole of \(\mathrm{Hg}\) atoms \(\left(V=4 \pi r^{3} / 3\right)\). (d) From your answers to (a), (b), and (c), calculate the percentage of the total volume occupied by the atoms in \(\mathrm{Hg}(l)\) and \(\mathrm{Hg}(g)\) at \(20^{\circ} \mathrm{C}\) and \(1.2 \times 10^{-3} \mathrm{~mm} \mathrm{Hg}\)

19\. Argon gas has its triple point at \(-189.3^{\circ} \mathrm{C}\) and \(516 \mathrm{~mm} \mathrm{Hg}\). It has a critical point at \(-122^{\circ} \mathrm{C}\) and \(48 \mathrm{~atm}\). The density of the solid is \(1.65 \mathrm{~g} / \mathrm{cm}^{3}\) whereas that of the liquid is \(1.40 \mathrm{~g} / \mathrm{cm}^{3}\). Sketch the phase diagram for argon and use it to fill in the blanks below with the words "boils" "melts" "sublimes," or "condenses." (a) Solid argon at \(500 \mathrm{~mm} \mathrm{Hg} \) when the temperature is increased. (b) Solid argon at 2 atm increased. (c) Argon gas at \(-150^{\circ} \mathrm{C}\) when the pressure is increased. (d) Argon gas at \(-165^{\circ} \mathrm{C} \) when the pressure is increased.

The vapor pressure of \(\mathrm{I}_{2}(s)\) at \(30^{\circ} \mathrm{C}\) is \(0.466 \mathrm{~mm} \mathrm{Hg}\). (a) How many milligrams of iodine will sublime into an evacuated 1.00-L flask? (b) If \(2.0 \mathrm{mg}\) of \(\mathrm{I}_{2}\) is used, what will the final pressure be? (c) If \(10.0 \mathrm{mg}\) of \(\mathrm{I}_{2}\) is used, what will the final pressure be?

The data below give the vapor pressure of octane, a major component of gasoline. \(\begin{array}{lllcl}\text { vp }(\mathrm{mm} \mathrm{Hg}) & 10 & 40 & 100 & 400 \\ t\left({ }^{\circ} \mathrm{C}\right) & 19.2 & 45.1 & 65.7 & 104.0\end{array}\) Plot ln vp versus \(1 / T\). Use your graph to estimate the heat of vaporization of octane. \(\left(\ln P=A-\frac{\Delta H_{\mathrm{vap}}}{R}\left(\frac{1}{T}\right)\right.\), where \(A\) is the \(y\) -intercept and \(\Delta H_{\mathrm{vap}}\) is the slope.)

Given the following data about xenon, $$ \begin{aligned} &\text { normal boiling point }=-108^{\circ} \mathrm{C} \\ &\text { normal melting point }=-112^{\circ} \mathrm{C} \\ &\text { triple point }=-121^{\circ} \mathrm{C} \text { at } 281 \mathrm{~mm} \mathrm{Hg} \\ &\text { critical point }=16.6^{\circ} \mathrm{C} \text { at } 58 \mathrm{~atm} \end{aligned} $$ (a) Construct an approximate phase diagram for xenon. (b) Estimate the vapor pressure of xenon at \(-115^{\circ} \mathrm{C}\). (c) Is the density of solid Xe larger than that for liquid Xe?
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