What is the volume of 10.0 grams of water vapor at 134.5 degrees Celsius and a pressure of 567 torr?
Understand the Problem
The question is asking to calculate the volume of water vapor given its mass, temperature, and pressure. We will use the Ideal Gas Law (PV=nRT) to solve for the volume (V). We will first need to convert the given values into appropriate units (grams to moles, Celsius to Kelvin, and torr to atm) before applying the formula.
Answer
24.8 L
The volume of 10.0 grams of water vapor at 134.5 degrees Celsius and a pressure of 567 torr is approximately 24.8 L.
Answer for screen readers
The volume of 10.0 grams of water vapor at 134.5 degrees Celsius and a pressure of 567 torr is approximately 24.8 L.
More Information
The ideal gas law is an equation of state of a hypothetical ideal gas. It is a good approximation of the behavior of many gases under many conditions, although it has several limitations.
Tips
Ensure all units are consistent with the ideal gas constant R (0.0821 L atm / (mol K)). Convert pressure to atmospheres and temperature to Kelvin.
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