Chapter 8: Problem 6
If you put a drinking straw in water, place your finger over the opening, and lift the straw out of the water, some water stays in the straw. Explain.
/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none}
Learning Materials
Features
Discover
Chapter 8: Problem 6
If you put a drinking straw in water, place your finger over the opening, and lift the straw out of the water, some water stays in the straw. Explain.
All the tools & learning materials you need for study success - in one app.
Get started for free
Calculate the pressure exerted by \(0.5000\) mole of \(\mathrm{N}_{2}\) in a \(1.0000-\mathrm{L}\) container at \(25.0^{\circ} \mathrm{C}\) a. using the ideal gas law. b. using the van der Waals equation. c. Compare the results.
Consider a \(1.0\) -\(\mathrm{L}\) container of neon gas at STP. Will the average kinetic energy, average velocity, and frequency of collisions of gas molecules with the walls of the container increase, decrease, or remain the same under each of the following conditions? a. The temperature is increased to \(100^{\circ} \mathrm{C}\) b. The temperature is decreased to \(-50^{\circ} \mathrm{C}\) c. The volume is decreased to \(0.5 \mathrm{L}\) d. The number of moles of neon is doubled.
At room temperature, water is a liquid with a molar volume of 18 mL. At \(105^{\circ} \mathrm{C}\) and 1 atm pressure, water is a gas and has a molar volume of over 30 L. Explain the large difference in molar volumes.
Calculate \(w\) and \(\Delta E\) when \(1\) mole of a liquid is vaporized at its boiling point \(\left(80 .^{\circ} \mathrm{C}\right)\) and \(1.00\) atm pressure. \(\Delta H\) for the vaporization of the liquid is \(30.7 \mathrm{kJ} / \mathrm{mol}\) at \(80 .^{\circ} \mathrm{C}\). Assume the volume of \(1\) mole of liquid is negligible as compared to the volume of \(1\) mole of gas at \(80 .^{\circ} \mathrm{C}\) and \(1.00\) atm.
Complete the following table for an ideal gas. $$\begin{aligned} &-\\\ &\begin{array}{|llll|} \hline {P} & {V} & {n} & {\boldsymbol{T}} \\ \hline 7.74 \times 10^{3} \mathrm{Pa} & 12.2 \mathrm{mL} & & 25^{\circ} \mathrm{C} \\ \hline & 43.0 \mathrm{mL} & 0.421 \mathrm{mol} & 223 \mathrm{K} \\ \hline 455 \text { torr } & & 4.4 \times 10^{-2} \mathrm{mol} & 331^{\circ} \mathrm{C} \\ \hline 745 \mathrm{mm} \mathrm{Hg} & 11.2 \mathrm{L} & 0.401 \mathrm{mol} & \\ \hline \end{array} \end{aligned}$$
What do you think about this solution?
We value your feedback to improve our textbook solutions.