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(a) What volume of air at 1.0 atm and \(22^{\circ} \mathrm{C}\) is needed to fill a \(0.98-\mathrm{L}\) bicycle tire to a pressure of \(5.0 \mathrm{~atm}\) at the same temperature? (Note that the 5.0 atm is the gauge pressure, which is the difference between the pressure in the tire and atmospheric pressure. Before filling, the pressure in the tire was \(1.0 \mathrm{~atm} .\) ) (b) What is the total pressure in the tire when the gauge pressure reads 5.0 atm? (c) The tire is pumped by filling the cylinder of a hand pump with air at 1.0 atm and then, by compressing the gas in the cylinder, adding all the air in the pump to the air in the tire. If the volume of the pump is 33 percent of the tire's volume, what is the gauge pressure in the tire after three full strokes of the pump? Assume constant temperature.

Short Answer

Expert verified
(a) 5.88 L of air is needed; (b) Total pressure is 6 atm; (c) Gauge pressure after 3 strokes is 3.01 atm.

Step by step solution

01

Understanding the Problem and Initial Conditions

First, we need to determine the volumes and pressures involved. Initially, the bicycle tire has a volume of 0.98 L and is filled to a pressure of 1 atm. We aim to increase the total pressure in the tire to a gauge pressure of 5 atm, which is actually 6 atm total, since we add 1 atm (atmospheric pressure).
02

Calculating Air Volume to Fill Tire

Using Boyle's Law, where the initial state is air at 1 atm and 22°C (V₁, P₁ = 1 atm), and the final state is air in a 0.98 L tire at 6 atm:\[ P_1V_1 = P_2V_2 \]Insert values: \(1 \text{ atm} \times V_1 = 6 \text{ atm} \times 0.98 \text{ L}\)Solve for \(V_1\):\[ V_1 = \frac{6 \times 0.98}{1} = 5.88 \text{ L} \]Thus, 5.88 L of air at 1 atm and 22°C is required to fill the tire.
03

Calculating Total Pressure in Tire

Gauge pressure reads 5 atm, adding atmospheric pressure, total pressure becomes:\[ P_{total} = P_{gauge} + P_{atm} = 5 + 1 = 6 \text{ atm} \]
04

Volume of Pump and Number of Strokes

The pump's volume is 33% of the tire's volume. Calculate pump volume:\[ V_{pump} = 0.33 \times V_{tire} = 0.33 \times 0.98 = 0.3234 \text{ L} \]Each pump stroke adds 0.3234 L of air at 1 atm to the tire.
05

Calculating New Pressure in Tire After Three Strokes

After three strokes, we add the volume of air from the pump 3 times, each time at 1 atm, to the tire:Total volume added after 3 strokes is:\[ V_{added} = 3 \times V_{pump} = 3 \times 0.3234 = 0.9702 \text{ L} \]Total volume of air in tire:\[ V_{total} = 0.98 \text{ L} + 0.9702 \text{ L} = 1.9502 \text{ L} \]Using Boyle's Law, calculate new gauge pressure:\[ P_2 = \left( \frac{6 \text{ atm} \times 0.98 \text{ L}}{1.9502 \text{ L}} \right) - 1 \text{ atm} \]Solve:\[ P_2 = \left( \frac{5.88}{1.9502} \right) - 1 = 3.014 \text{ atm} \]
06

Conclusion

The total pressure in the tire after three full pump strokes, maintaining constant temperature, results in a gauge pressure of approximately 3.01 atm.

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Key Concepts

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

Gas Laws
Gas laws are fundamental in understanding how gases behave under different conditions. One of the most important is **Boyle's Law**, which describes the relationship between pressure and volume. It states that at a constant temperature for a fixed amount of gas, pressure is inversely proportional to volume. This means as pressure increases, volume decreases, and vice versa. It's mathematically represented as:\[ P_1V_1 = P_2V_2 \]Here,
  • \( P_1 \) and \( V_1 \) are the initial pressure and volume, respectively.
  • \( P_2 \) and \( V_2 \) are the final pressure and volume.
Understanding this law is crucial to solving problems like filling a bicycle tire, where we need to calculate how the volume of gas changes as we compress it into the tire. It's about balancing pressure and volume, always ensuring that when one changes, the other counters it to maintain equilibrium.
Pressure Calculation
Pressure calculation is a key step in working with gases. It's important to distinguish between **gauge pressure** and **total pressure**. Gauge pressure is the extra pressure in a system over atmospheric pressure, while total pressure includes both atmospheric and gauge pressures. In our exercise:
  • Gauge pressure is given as 5 atm.
  • Atmospheric pressure is approximately 1 atm.
Thus, the total pressure becomes:\[ P_{total} = P_{gauge} + P_{atm} \]For a tight fit to work right, calculating the total pressure helps ensure that the tire does not burst from too much pressure. Knowing the total pressure allows us to determine how much air is needed and how it adjusts the actual physical state of the tire.
Temperature
Temperature is a vital component in gas behavior but interestingly does not change in this problem, making analysis simpler. This is known as the **isothermal process**, where the gas temperature remains constant throughout the procedure. In our exercise:- The temperature is held at \(22^{\circ} C\). - This stability allows us to focus solely on the interplay between pressure and volume without worrying about temperature fluctuations changing the dynamics.When temperature remains constant, Boyle's Law can be directly applied without modifications for temperature changes, simplifying our calculations and yielding clear results.
Volume Expansion
Volume expansion is a key concept in gas laws applied to real-world scenarios like filling a tire. It's about understanding how added air volume affects an enclosed space. In the exercise: - Air from the pump is repeatedly added to increase the total air volume in the tire. - Each pump stroke introduces additional air, expanding the volume of gas inside the tire. The pump's volume is calculated as 33% of the tire's volume. Thus each pump action significantly impacts the tire's volume and pressure:
  • Volume per stroke: 0.3234 L is added.
  • After three strokes, approximately 0.9702 L is added.
Remember, as volume increases, unless the container's capacity is exceeded, pressure should theoretically decrease, according to Boyle's Law, unless we add more air to counterbalance this expansion. By understanding volume expansion, we control how gas behaves, ensuring that a tire inflates correctly and safely.

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Most popular questions from this chapter

A stockroom supervisor measured the contents of a 25.0-gal drum partially filled with acetone on a day when the temperature was \(18.0^{\circ} \mathrm{C}\) and atmospheric pressure was \(750 \mathrm{mmHg}\), and found that 15.4 gal of the solvent remained. After tightly sealing the drum, an assistant dropped the drum while carrying it upstairs to the organic laboratory. The drum was dented, and its internal volume was decreased to 20.4 gal. What is the total pressure inside the drum after the accident? The vapor pressure of acetone at \(18.0^{\circ} \mathrm{C}\) is \(400 \mathrm{mmHg}\). (Hint: At the time the drum was sealed, the pressure inside the drum, which is equal to the sum of the pressures of air and acetone, was equal to the atmospheric pressure.)

A student breaks a thermometer and spills most of the mercury (Hg) onto the floor of a laboratory that measures \(15.2 \mathrm{~m}\) long, \(6.6 \mathrm{~m}\) wide, and \(2.4 \mathrm{~m}\) high. (a) Calculate the mass of mercury vapor (in grams) in the room at \(20^{\circ} \mathrm{C}\). The vapor pressure of mercury at \(20^{\circ} \mathrm{C}\) is \(1.7 \times 10^{-6}\) atm. (b) Does the concentration of mercury vapor exceed the air quality regulation of \(0.050 \mathrm{mg} \mathrm{Hg} / \mathrm{m}^{3}\) of air? (c) One way to deal with small quantities of spilled mercury is to spray sulfur powder over the metal. Suggest a physical and a chemical reason for this action.

A sample of zinc metal reacts completely with an excess of hydrochloric acid: $$ \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) $$ The hydrogen gas produced is collected over water at \(25.0^{\circ} \mathrm{C}\) using an arrangement similar to that shown in Figure \(10.14(\mathrm{a})\). The volume of the gas is \(7.80 \mathrm{~L},\) and the pressure is 0.980 atm. Calculate the amount of zinc metal in grams consumed in the reaction. (Vapor pressure of water at \(\left.25^{\circ} \mathrm{C}=23.8 \mathrm{mmHg} .\right)\)

The apparatus shown here can be used to measure atomic and molecular speeds. Suppose that a beam of metal atoms is directed at a rotating cylinder in a vacuum. A small opening in the cylinder allows the atoms to strike a target area. Because the cylinder is rotating, atoms traveling at different speeds will strike the target at different positions. In time, a layer of the metal will deposit on the target area, and the variation in its thickness is found to correspond to Maxwell's speed distribution. In one experiment it is found that at \(850^{\circ} \mathrm{C}\) some bismuth (Bi) atoms struck the target at a point \(2.80 \mathrm{~cm}\) from the spot directly opposite the slit. The diameter of the cylinder is \(15.0 \mathrm{~cm},\) and it is rotating at 130 revolutions per second. (a) Calculate the speed (in \(\mathrm{m} / \mathrm{s}\) ) at which the target is moving. (Hint: The circumference of a circle is given by \(2 \pi r\), where \(r\) is the radius.) (b) Calculate the time (in seconds) it takes for the target to travel \(2.80 \mathrm{~cm} .\) (c) Determine the speed of the \(\mathrm{Bi}\) atoms. Compare your result in part (c) with the \(u_{\mathrm{rms}}\) of \(\mathrm{Bi}\) at \(850^{\circ} \mathrm{C}\). Comment on the difference.

What is the mass of the solid \(\mathrm{NH}_{4} \mathrm{Cl}\) formed when \(73.0 \mathrm{~g}\) of \(\mathrm{NH}_{3}\) is mixed with an equal mass of \(\mathrm{HCl} ?\) What is the volume of the gas remaining, measured at \(14.0^{\circ} \mathrm{C}\) and \(752 \mathrm{mmHg}\) ? What gas is it?

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