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Chapter 10: Problem 1

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 the significantly lower atmospheric pressure on Mars (\(0.007\) atm) compared to Earth (1 atm). This lower pressure means there will be less force pushing the liquid up the straw on Mars, making it more difficult to drink.

Step by step solution

01

(Compare Atmospheric Pressures)

(To determine the ease of drinking from a straw on Mars compared to Earth, we need to compare their average atmospheric pressures. The atmospheric pressure on Earth is generally considered to be 1 atm, while the atmospheric pressure on Mars is given to be 0.007 atm.) #Step 2: Analyze Pressure Difference Requirements#
02

(Analyze Pressure Difference Requirements)

(To drink from a straw, a person creates a pressure difference by sucking the air out of the straw. The liquid is then pushed up into the straw by the atmospheric pressure acting on its surface. Higher atmospheric pressure means a greater force pushing the liquid up the straw.) #Step 3: Determine Drinking Ease Based On Pressure Differences#
03

(Determine Drinking Ease Based On Pressure Differences)

(As we know, the atmospheric pressure on Earth is 1 atm, which is significantly greater than the 0.007 atm pressure on Mars. This means that there will be less force pushing the liquid up the straw on Mars compared to Earth. Thus, it would be harder to drink from a straw on Mars than on Earth.)

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Most popular questions from this chapter

A piece of dry ice (solid carbon dioxide) with a mass of \(5.50 \mathrm{~g}\) is placed in a \(10.0\) - \(L\) vessel that already contains air at 705 torr and \(24^{\circ} \mathrm{C}\). After the carbon dioxide has totally sublimed, what is the partial pressure of the resultant \(\mathrm{CO}_{2}\) gas, and the total pressure in the container at \(24^{\circ} \mathrm{C}\) ?

Does the effect of intermolecular attraction on the properties of a gas become more significant or less significant if (a) the gas is compressed to a smaller volume at constant temperature; (b) the temperature of the gas is increased at constant volume?

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Assume that an exhaled breath of air consists of \(74.8 \% \mathrm{~N}_{2}, 15.3 \% \mathrm{O}_{2}, 3.7 \% \mathrm{CO}_{2}\), and \(6.2 \%\) water vapor. (a) If the total pressure of the gases is \(0.985 \mathrm{~atm}\), calculate the partial pressure of each component of the mixture. (b) If the volume of the exhaled gas is \(455 \mathrm{~mL}\) and its temperature is \(37^{\circ} \mathrm{C}\), calculate the number of moles of \(\mathrm{CO}_{2}\) exhaled. (c) How many grams of glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) would need to be metabolized to produce this quantity of \(\mathrm{CO}_{2}\) ? (The chemical reaction is the same as that for combustion of \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\). See Section \(3.2\) and Problem 10.57.)

Chlorine is widely used to purify municipal water supplies and to treat swimming pool waters. Suppose that the volume of a particular sample of \(\mathrm{Cl}_{2}\) gas is \(8.70 \mathrm{~L}\) at 895 torr and \(24^{\circ} \mathrm{C}\). (a) How many grams of \(\mathrm{Cl}_{2}\) are in the sample? (b) What volume will the \(\mathrm{Cl}_{2}\) occupy at STP? (c) At what temperature will the volume be \(15.00 \mathrm{~L}\) if the pressure is \(8.76 \times 10^{2}\) torr? (d) At what pressure will the volume equal \(5.00 \mathrm{~L}\) if the temperature is \(58^{\circ} \mathrm{C}\) ?
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