A force of 2.31 * 10^4 N is applied to a diver’s face mask that has an area of 125 cm^2. Find the pressure in atm on the face mask.

Verified step by step guidance

Convert the area from cm² to m² by using the conversion factor 1 m² = 10,000 cm². This is done by dividing the area in cm² by 10,000.

Calculate the pressure in pascals (Pa) using the formula: Pressure (P) = Force (F) / Area (A).

Convert the pressure from pascals to atmospheres (atm) using the conversion factor 1 atm = 101,325 Pa. This is done by dividing the pressure in pascals by 101,325.

Ensure all units are consistent throughout the calculations to avoid any errors in the final result.

Check the calculation for accuracy by reviewing each step and ensuring that all mathematical operations are performed correctly.

Key Concepts

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

Pressure

Pressure is defined as the force applied per unit area. It is a measure of how much force is exerted on a given surface area and is typically expressed in units such as pascals (Pa) or atmospheres (atm). In this context, pressure can be calculated using the formula P = F/A, where P is pressure, F is force, and A is area.

Unit Conversion

In chemistry and physics, it is often necessary to convert units to ensure consistency in calculations. In this problem, the area is given in square centimeters (cm²), which must be converted to square meters (m²) to match the SI unit system. Additionally, the final pressure needs to be converted from pascals to atmospheres, where 1 atm is equivalent to 101,325 Pa.

Atmospheric Pressure

Atmospheric pressure is the pressure exerted by the weight of the atmosphere at a given point and is commonly used as a reference point in various calculations. Standard atmospheric pressure at sea level is defined as 1 atm, which is equivalent to 101,325 pascals. Understanding this concept is crucial for interpreting the results of pressure calculations in relation to everyday experiences.

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Textbook Question

Mercury is often used in thermometers. The mercury sits in a bulb on the bottom of the thermometer and rises up a thin capillary as the temperature rises. Suppose a mercury thermometer contains 3.380 g of mercury and has a capillary that is 0.200 mm in diameter. How far does the mercury rise in the capillary when the temperature changes from 0.0 °C to 25.0 °C? The density of mercury at these temperatures is 13.596 g/cm³ and 13.534 g/cm³, respectively

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