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Mars has an average atmospheric pressure of \(0.007\) atm. 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 harder to drink from a straw on Mars than on Earth due to Mars' lower atmospheric pressure (0.007 atm). The lower pressure would require a greater pressure difference between the inside of the mouth and the Mars atmosphere in order to draw liquid up the straw.

Step by step solution

01

Understanding Atmospheric Pressure on Earth

On Earth, the atmospheric pressure is about 1 atmosphere (atm). Drinking from a straw relies on creating a pressure difference between the inside of the mouth and the atmosphere. When we drink, we create a partial vacuum in our mouth by sucking the air out of the straw. This reduces the pressure in the straw and allows the surrounding atmospheric pressure to push the liquid up the straw and into our mouth.
02

Comparing Atmospheric Pressure on Mars

Mars has an average atmospheric pressure of 0.007 atm, which is significantly lower than the atmospheric pressure on Earth. To determine whether it would be easier or harder to drink from a straw on Mars, we need to evaluate the effect of this lower atmospheric pressure on the ability to create a pressure difference and draw liquid through the straw.
03

Considering the Pressure Difference

On Earth, the atmospheric pressure helps push the liquid up the straw when a vacuum is created inside the mouth. However, on Mars, with its lower atmospheric pressure, the force exerted by the atmosphere on the liquid is weaker. This means that a greater pressure difference between the inside of the mouth and the Mars atmosphere would need to be created to overcome the reduced atmospheric pressure and draw the liquid up the straw.
04

Conclusion

Due to the lower atmospheric pressure on Mars (0.007 atm), it would be harder to drink from a straw compared to Earth. This is because the reduced pressure would require a greater pressure difference between the inside of the mouth and the Mars atmosphere in order to draw liquid up the straw.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Mars Atmosphere
Mars is often referred to as the "Red Planet," not just for its surface color but for the intriguing aspects of its atmosphere. Understanding its atmosphere presents an exciting challenge for scientists and enthusiasm for learners like us.
  • The Martian atmosphere is thin, with an average pressure of only 0.007 atm, which is just a fraction of Earth's 1 atm.
  • This extremely low pressure is due to Mars' weaker gravity and the loss of its atmosphere over billions of years.
  • The atmosphere is mostly composed of carbon dioxide, with minor amounts of nitrogen and argon, and traces of water vapor and oxygen.
Due to this low pressure, physical phenomena we take for granted on Earth, such as drinking through a straw, function very differently. Exploring the intricacies of the Martian atmosphere can help us understand why these differences occur.
Pressure Difference
Pressure difference is a fundamental concept in understanding how fluids move from one place to another. This concept is pivotal when considering drinking through a straw.
  • On Earth, atmospheric pressure is our helper, exerting a force that pushes liquid up when we create a low-pressure area in our mouth by sucking air out of the straw.
  • The larger the pressure difference between the inside of the straw and the outside atmosphere, the easier it is for the liquid to move upwards.
Comparing this to Mars, where atmospheric pressure is only 0.007 atm, creating a similar pressure difference is challenging. The minuscule atmospheric pressure provides less force to push the liquid, meaning one needs to suck even harder to achieve the same effect as on Earth. The pressure difference requirement is enhanced on Mars due to the feeble atmospheric pressure, making simple tasks like drinking from a straw much harder.
Liquid Dynamics
Liquid dynamics involves the study of fluid motion and the forces influencing it, crucial for understanding how and why liquids behave differently in various environments.
  • In environments like Earth, liquid dynamics are heavily influenced by atmospheric pressure, gravity, and the properties of the liquid itself.
  • Liquids flow from areas of higher pressure to lower pressure, which is why creating a pressure difference is essential for sucking a drink through a straw.
On Mars, the dynamics change due to the low atmospheric pressure. The reduced force applied on the liquid means you need to create a significant enough pressure difference within the straw to compensate for the lack of environmental pressure. This introduces unique challenges, as less atmospheric pressure implies less assistance in overcoming gravity to move the liquid upward. Understanding liquid dynamics on Mars reveals much about the inventive engineering required for tasks that are mundane on Earth.

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Most popular questions from this chapter

Chlorine dioxide gas \(\left(\mathrm{ClO}_{2}\right)\) is used as a commercial bleaching agent. It bleaches materials by oxidizing them. In the course of these reactions, the \(\mathrm{ClO}_{2}\) is itself reduced. (a) What is the Lewis structure for \(\mathrm{ClO}_{2}\) ? (b) Why do you think that \(\mathrm{ClO}_{2}\) is reduced so readily? (c) When a \(\mathrm{ClO}_{2}\) molecule gains an electron, the chlorite ion, \(\mathrm{ClO}_{2}^{-}\), forms. Draw the Lewis structure for \(\mathrm{ClO}_{2}^{-}\). (d) Predict the \(\mathrm{O}-\mathrm{Cl}-\mathrm{O}\) bond angle in the \(\mathrm{ClO}_{2}^{-}\) ion. (e) One method of preparing \(\mathrm{ClO}_{2}\) is by the reaction of chlorine and sodium chlorite: $$ \mathrm{Cl}_{2}(g)+2 \mathrm{NaClO}_{2}(s) \longrightarrow 2 \mathrm{ClO}_{2}(g)+2 \mathrm{NaCl}(s) $$ If you allow \(10.0 \mathrm{~g}\) of \(\mathrm{NaClO}_{2}\) to react with \(2.00 \mathrm{~L}\) of chlorine gas at a pressure of \(1.50 \mathrm{~atm}\) at \(21^{\circ} \mathrm{C}\), how many grams of \(\mathrm{ClO}_{2}\) can be prepared?

What property or properties of gases can you point to that support the assumption that most of the volume in a gas is empty space?

A fixed quantity of gas at \(21^{\circ} \mathrm{C}\) exhibits a pressure of 752 torr and occupies a volume of \(4.38 \mathrm{~L}\). (a) Use Boyle's law to calculate the volume the gas will occupy if the pressure is increased to \(1.88\) atm while the temperature is held constant. (b) Use Charles's law to calculate the volume the gas will occupy if the temperature is increased to \(175^{\circ} \mathrm{C}\) while the pressure is held constant.

Magnesium can be used as a "getter" in evacuated enclosures, to react with the last traces of oxygen. (The magnesium is usually heated by passing an electric current through a wire or ribbon of the metal.) If an enclosure of \(0.382 \mathrm{~L}\) has a partial pressure of \(\mathrm{O}_{2}\) of \(3.5 \times 10^{-6}\) torr at \(27{ }^{\circ} \mathrm{C}\), what mass of magnesium will react according to the following equation? $$ 2 \mathrm{Mg}(s)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{MgO}(s) $$

Which of the following statements best explains why nitrogen gas at STP is less dense than Xe gas at STP? (a) Because Xe is a noble gas, there is less tendency for the Xe atoms to repel one another, so they pack more densely in the gas state. (b) Xe atoms have a higher mass than \(\mathrm{N}_{2}\) molecules. Because both gases at STP have the same number of molecules per unit volume, the Xe gas must be denser. (c) The Xe atoms are larger than \(\mathrm{N}_{2}\) molecules and thus take up a larger fraction of the space occupied by the gas. (d) Because the Xe atoms are much more massive than the \(\mathrm{N}_{2}\) molecules, they move more slowly and thus exert less upward force on the gas container and make the gas appear denser.

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