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Ch.10 - Gases
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoBrown 14th EditionCh.10 - GasesProblema 97
Capitolo 10, Problema 97

Torricelli, who invented the barometer, used mercury in its construction because mercury has a very high density, which makes it possible to make a more compact barometer than one based on a less dense fluid. Calculate the density of mercury using the observation that the column of mercury is 760 mm high when the atmospheric pressure is 1.01 * 105 Pa. Assume the tube containing the mercury is a cylinder with a constant cross-sectional area.

Guida verificata passo dopo passo
1
Step 1: Understand that the pressure at the base of a fluid column is given by the equation P = ρgh, where P is the pressure, ρ is the density of the fluid, g is the acceleration due to gravity, and h is the height of the fluid column.
Step 2: In this problem, we are given P (atmospheric pressure = 1.01 * 10^5 Pa), g (acceleration due to gravity = 9.8 m/s^2), and h (height of the mercury column = 760 mm = 0.76 m). We are asked to solve for ρ (density of mercury).
Step 3: Rearrange the equation P = ρgh to solve for ρ. The rearranged equation is ρ = P / (gh).
Step 4: Substitute the given values into the rearranged equation. ρ = (1.01 * 10^5 Pa) / (9.8 m/s^2 * 0.76 m).
Step 5: Calculate the density of mercury by performing the division in the equation from step 4. This will give you the density of mercury in kg/m^3.

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Density

Density is defined as mass per unit volume, typically expressed in grams per cubic centimeter (g/cm³) or kilograms per cubic meter (kg/m³). It is a fundamental property of materials that influences how substances behave under various conditions. In the context of the barometer, the high density of mercury allows for a shorter column height compared to less dense fluids, making it practical for measuring atmospheric pressure.
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Atmospheric Pressure

Atmospheric pressure is the force exerted by the weight of the air above a given point, measured in pascals (Pa) or millimeters of mercury (mmHg). At sea level, standard atmospheric pressure is approximately 101,325 Pa, which corresponds to a mercury column height of 760 mm. This relationship is crucial for understanding how barometers function, as they measure changes in atmospheric pressure by the height of the mercury column.
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Hydrostatic Pressure

Hydrostatic pressure is the pressure exerted by a fluid at equilibrium due to the force of gravity. It is calculated using the formula P = ρgh, where P is the pressure, ρ is the fluid density, g is the acceleration due to gravity, and h is the height of the fluid column. In the case of the barometer, the hydrostatic pressure of the mercury column balances the atmospheric pressure, allowing for the calculation of mercury's density based on the height of the column.
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Calculate the pressure that CCl4 will exert at 80 °C if 1.00 mol occupies 33.3 L, assuming that (a) CCl4 obeys the ideal-gas equation (b) CCl4 obeys the van der Waals equation. (Values for the van der Waals constants are given in Table 10.3.)

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Calculate the pressure that CCl4 will exert at 80 °C if 1.00 mol occupies 33.3 L, assuming that (c) Which would you expect to deviate more from ideal behavior under these conditions, Cl2 or CCl4? Explain.

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Table 10.3 shows that the van der Waals b parameter has units of L/mol. This means that we can calculate the sizes of atoms or molecules from the b parameter. Refer back to the discussion in Section 7.3. Is the van der Waals radius we calculate from the b parameter of Table 10.3 more closely associated with the bonding or nonbonding atomic radius discussed there? Explain.

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