Ch.10 - Gases

Brown - Chemistry: The Central Science 15th Edition

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Brown 15th Edition

Ch.10 - Gases

Problem 19c

Chapter 10, Problem 19c

The typical atmospheric pressure on top of Mount Everest (29,032 ft) is about 265 torr. Convert this pressure to c. pascals,

Verified step by step guidance

Start by understanding the relationship between different pressure units. We know that 1 atm = 760 torr and 1 atm = 101325 pascals.

Set up a conversion factor to convert from torr to atm. Use the relationship: \( \text{Pressure in atm} = \frac{\text{Pressure in torr}}{760} \).

Convert the given pressure from torr to atm using the conversion factor: \( \text{Pressure in atm} = \frac{265}{760} \).

Now, convert the pressure from atm to pascals using the relationship: \( \text{Pressure in pascals} = \text{Pressure in atm} \times 101325 \).

Multiply the pressure in atm by 101325 to find the pressure in pascals.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Pressure Units

Pressure is a measure of force applied per unit area, commonly expressed in various units such as torr, pascals (Pa), and atmospheres (atm). Understanding these units is crucial for converting between them, as each unit represents a different scale of measurement. For instance, 1 torr is defined as 1/760 of an atmosphere, while 1 pascal is defined as one newton per square meter.

Conversion Factors

Conversion factors are numerical values used to convert a quantity from one unit to another. In the context of pressure, knowing the relationship between torr and pascals is essential for accurate conversions. Specifically, 1 torr is equivalent to approximately 133.322 pascals, which allows for straightforward calculations when converting atmospheric pressure values.

Atmospheric Pressure

Atmospheric pressure is the force exerted by the weight of air above a given point, typically measured at sea level. It decreases with altitude, which is why the pressure on Mount Everest is significantly lower than at sea level. Understanding how atmospheric pressure varies with elevation is important for interpreting pressure readings in different geographical locations.

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Textbook Question

(a) The compound 1-iodododecane is a nonvolatile liquid with a density of 1.20 g>mL. The density of mercury is 13.6 g>mL. What do you predict for the height of a barometer column based on 1-iodododecane, when the atmospheric pressure is 749 torr?

The typical atmospheric pressure on top of Mount Everest (29,032 ft) is about 265 torr. Convert this pressure to d. bars,

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Textbook Question

How high in meters must a column of glycerol be to exert a pressure equal to that of a 760-mm column of mercury? The density of glycerol is 1.26 g/mL, whereas that of mercury is 13.6 g/mL.

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Textbook Question

What pressure, in atmospheres, is exerted on the body of a diver if they are 15 ft below the surface of the water when the atmospheric pressure is 750 torr? Assume that the density of the water is 1.00 g/cm3=1.00×103 kg/m3. The gravitational constant is 9.81 m/s2, and 1 Pa=1 kg/m-s2.

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Textbook Question

Perform the following conversions: (d) 1.323 * 105 Pa to atmospheres

615

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