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Chapter 10: Problem 1

Mars has an average atmospheric pressure of 709 pa. Would it be easier or harder to drink from a straw on Mars than on Earth? Explain. [Section 10.2\(]\)

Short Answer

Expert verified
It would be easier to drink from a straw on Mars compared to Earth because the atmospheric pressure on Mars (709 Pa) is much lower than that on Earth (101325 Pa). Creating a "partial vacuum" within the straw while drinking requires less effort on Mars, allowing liquid to flow more easily due to the lower external atmospheric pressure.

Step by step solution

01

Compare atmospheric pressures on Mars and Earth

Compare the atmospheric pressure on Mars (709 Pa) to that of Earth (101325 Pa). We can see that Earth's atmospheric pressure is much higher than Mars'.
02

Understand how a straw works

When you drink from a straw, you create an area of lower pressure inside the straw by removing air and making a "partial vacuum." This difference in pressure causes the liquid at the bottom of the straw to be pushed up by the greater atmospheric pressure outside of the straw, allowing you to drink the liquid.
03

Compare the pressure needed to create a vacuum in the straw on Mars vs Earth

Let's compare the pressure that needs to be created inside the straw on Mars and Earth to overcome the external atmospheric pressure. On Earth, the pressure inside the straw should be significantly less than the atmospheric pressure (101325 Pa) to allow liquid to flow. On Mars, the pressure inside the straw needs to be lower than the atmospheric pressure of 709 Pa.
04

Determine the ease of drinking from a straw on Mars compared to Earth

Since the atmospheric pressure is much lower on Mars (709 Pa) than on Earth (101325 Pa), it would require less effort to create the "partial vacuum" within the straw while drinking. This means that it would be easier to drink from a straw on Mars compared to Earth due to the lower atmospheric pressure.

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Most popular questions from this chapter

An 8.40 -g sample of argon and an unknown mass of \(\mathrm{H}_{2}\) are mixed in a flask at room temperature. The partial pressure of the argon is $44.0 \mathrm{kPa},\( and that of the hydrogen is \)57.33 \mathrm{kPa} .$ What is the mass of the hydrogen?

Ammonia and hydrogen chloride react to form solid ammonium chloride: $$\mathrm{NH}_{3}(g)+\mathrm{HCl}(g) \longrightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)$$ Two \(2.00-\mathrm{L}\) flasks at \(25^{\circ} \mathrm{C}\) are connected by a valve, as shown in the drawing. One flask contains \(5.00 \mathrm{~g}\) of \(\mathrm{NH}_{3}(g),\) and the other contains \(5.00 \mathrm{~g}\) of \(\mathrm{HCl}(g) .\) When the valve is opened, the gases react until one is completely consumed. (a) Which gas will remain in the system after the reaction is complete? (b) What will be the final pressure of the system after the reaction is complete? (Neglect the volume of the ammonium chloride formed.) (c) What mass of ammonium chloride will be formed?

A rigid vessel containing a \(3: 1 \mathrm{~mol}\) ratio of carbon dioxide and water vapor is held at \(200^{\circ} \mathrm{C}\) where it has a total pressure of \(202.7 \mathrm{kPa}\). If the vessel is cooled to \(10^{\circ} \mathrm{C}\) so that all of the water vapor condenses, what is the pressure of carbon dioxide? Neglect the volume of the liquid water that forms on cooling.

When a large evacuated flask is filled with argon gas, its mass increases by \(3.224 \mathrm{~g}\). When the same flask is again evacuated and then filled with a gas of unknown molar mass, the mass increase is 8.102 g. (a) Based on the molar mass of argon, estimate the molar mass of the unknown gas. \((\mathbf{b})\) What assumptions did you make in arriving at your answer?

In an experiment reported in the scientific literature, male cockroaches were made to run at different speeds on a miniature treadmill while their oxygen consumption was measured. In 30 minutes the average cockroach (running at \(0.08 \mathrm{~km} / \mathrm{h})\) consumed \(1.0 \mathrm{~mL}\) of \(\mathrm{O}_{2}\) at \(101.33 \mathrm{kPa}\) pressure and \(20^{\circ} \mathrm{C}\) per gram of insect mass. (a) How many moles of \(\mathrm{O}_{2}\) would be consumed in 1 day by a 6.3 -g cockroach moving at this speed? (b) This same cockroach is caught by a child and placed in a 2.0-L fruit jar with a tight lid. Assuming the same level of continuous activity as in the research, how much of the available \(\mathrm{O}_{2}\) will the cockroach consume in 1 day? (Air is \(21 \mathrm{~mol} \% \mathrm{O}_{2} .\) )
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