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Chapter 10: Problem 24

An open-end manometer containing mercury is connected to a container of gas, as depicted in Sample Exercise \(10.2\). What is the pressure of the enclosed gas in torr in each of the following situations? (a) The mercury in the arm attached to the gas is \(15.4 \mathrm{~mm}\) higher than in the one open to the atmosphere; atmospheric pressure is \(0.966\) atm. (b) The mercury in the arm attached to the gas is \(8.7 \mathrm{~mm}\) lower than in the one open to the atmosphere; atmospheric pressure is \(0.99\) atm.

Short Answer

Expert verified
The pressure of the enclosed gas in torr for case (a) is \(750.36 \ \text{torr}\), and for case (b) is \(743.7 \ \text{torr}\).

Step by step solution

01

Case (a): Mercury height in gas arm is higher

First, convert atmospheric pressure to torr: Atmospheric pressure = \(0.966 \ \text{atm}\) 1 atm = \(760 \ \text{torr}\) Atmospheric pressure = \(0.966 \times 760 \ \text{torr} = 734.96 \ \text{torr}\) Next, calculate pressure due to height difference of mercury: Height difference = \(15.4 \ \text{mm}\) 1 mmHg = 1 torr Pressure difference = \(15.4 \ \text{torr}\) Now, find the gas pressure in the container by adding the atmospheric pressure and the pressure difference: Gas pressure = atmospheric pressure + pressure difference = \(734.96 \ \text{torr} + 15.4 \ \text{torr} = 750.36 \ \text{torr}\)
02

Case (b): Mercury height in gas arm is lower

First, convert atmospheric pressure to torr: Atmospheric pressure = \(0.99 \ \text{atm}\) 1 atm = \(760 \ \text{torr}\) Atmosphere pressure = \(0.99 \times 760 \ \text{torr} = 752.4 \ \text{torr}\) Next, calculate pressure due to the height difference of mercury: Height difference = \(8.7 \ \text{mm}\) 1 mmHg = 1 torr Pressure difference = \(8.7 \ \text{torr}\) Now, find the gas pressure in the container by subtracting the pressure difference from the atmospheric pressure: Gas pressure = atmospheric pressure - pressure difference = \(752.4 \ \text{torr} - 8.7 \ \text{torr} = 743.7 \ \text{torr}\) Therefore, the pressure of the enclosed gas in torr for case (a) is 750.36 torr, and for case (b) is 743.7 torr.

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Key Concepts

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

Manometer
A manometer is a widely used device to measure gas pressure. It consists of a U-shaped tube filled with a liquid, commonly mercury. This tool can measure the difference in pressure between the gas in a container and the atmospheric pressure outside. Manometers can be open-end or closed-end.
Open-end manometers allow the liquid's free arm to be exposed to the atmosphere, whereas closed-end manometers have one end sealed.
When a gas is introduced to the manometer, it displaces the liquid vertically. These changes reflect differences in pressure.
  • If the liquid's level in the tube is higher on the side attached to the gas, the gas pressure is higher than the atmospheric pressure.
  • Conversely, if it's lower, the gas pressure is lower than the atmospheric pressure.
    These variations allow us to calculate the gas's precise pressure by considering the height difference in the liquid column.
Atmospheric Pressure Conversion
Atmospheric pressure is usually measured in atmospheres (atm), but other units like torr and millimeters of mercury (mmHg) are also common.
To solve problems involving manometers, we often need to convert atmospheric pressure to different units to match the units of the pressure difference.
The conversion between atmospheres and torr is straightforward because 1 atm is equal to 760 torr. This relationship is used to convert atmospheric pressure to torr, essential for calculations involving manometers. For example, converting 0.966 atm to torr involves multiplying by 760, resulting in approximately 734.96 torr.
  • Always ensure conversion accuracy to avoid errors in further calculations.
  • This conversion step is crucial before moving on to calculating pressure differences.
Pressure Difference Calculation
Calculating the pressure difference is a key step in determining the gas pressure inside a container using a manometer.
The pressure difference is derived from the height difference of the liquid column.
The relationship here is simple: 1 mmHg corresponds directly to 1 torr. This implies that a 15 mm difference in the mercury column equates to a 15 torr pressure difference.
By using this relation, we can:
  • Add the pressure difference to atmospheric pressure if the liquid level is higher on the side connected to the gas.
  • Subtract the pressure difference from atmospheric pressure if the liquid level is lower on the side attached to the gas.
    This step, along with atmospheric pressure conversion, allows for the precise computation of the gas's pressure.

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Most popular questions from this chapter

Suppose you are given two 1-L flasks and told that one contains a gas of molar mass 30 , the other a gas of molar mass 60 , both at the same temperature. The pressure in flask \(\mathrm{A}\) is \(\mathrm{X} \mathrm{atm}\), and the mass of gas in the flask is \(1.2 \mathrm{~g}\). The pressure in flask B is \(0.5 \mathrm{X} \mathrm{atm}\), and the mass of gas in that flask is \(1.2 \mathrm{~g}\). Which flask contains gas of molar mass 30 , and which contains the gas of molar mass 60 ?

Suppose you are given two flasks at the same temperature, one of volume \(2 \mathrm{~L}\) and the other of volume \(3 \mathrm{~L}\). The 2-L flask contains \(4.8 \mathrm{~g}\) of gas, and the gas pressure is \(X\) atm. The 3-L flask contains \(0.36 \mathrm{~g}\) of gas, and the gas pressure is \(0.1 \mathrm{X}\). Do the two gases have the same molar mass? If not, which contains the gas of higher molar mass?

A 6.53-g sample of a mixture of magnesium carbonate and calcium carbonate is treated with excess hydrochloric acid. The resulting reaction produces \(1.72 \mathrm{~L}\) of carbon dioxide gas at \(28^{\circ} \mathrm{C}\) and 743 torr pressure. (a) Write balanced chemical equations for the reactions that occur between hydrochloric acid and each component of the mixture. (b) Calculate the total number of moles of carbon dioxide that forms from these reactions. (c) Assuming that the reactions are complete, calculate the percentage by mass of magnesium carbonate in the mixture.

Indicate which of the following statements regarding the kinetic-molecular theory of gases are correct. For those that are false, formulate a correct version of the statement. (a) The average kinetic energy of a collection of gas molecules at a given temperature is proportional to \(\mathrm{m}^{1 / 2}\). (b) The gas molecules are assumed to exert no forces on each other. (c) All the molecules of a gas at a given temperature have the same kinetic energy. (d) The volume of the gas molecules is negligible in comparison to the total volume in which the gas is contained.

An herbicide is found to contain only \(C, H, N\), and \(C 1\) The complete combustion of a \(100.0-\mathrm{mg}\) sample of the herbicide in excess oxygen produces \(83.16 \mathrm{~mL}\) of \(\mathrm{CO}_{2}\) and \(73.30 \mathrm{~mL}\) of \(\mathrm{H}_{2} \mathrm{O}\) vapor at STP. A separate analysis shows that the sample also contains \(16.44 \mathrm{mg}\) of \(\mathrm{Cl}\). (a) Determine the percent composition of the substance. (b) Calculate its empirical formula.
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