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Ch.5 - Gases
All textbooksTro 4th EditionCh.5 - GasesProblem 123
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Chapter 5, Problem 123

A steel container of volume 0.35 L can withstand pressures up to 88 atm before exploding. What mass of helium can be stored in this container at 299 K?

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1
Identify the ideal gas law equation: \( PV = nRT \), where \( P \) is pressure, \( V \) is volume, \( n \) is the number of moles, \( R \) is the ideal gas constant, and \( T \) is temperature.
Rearrange the ideal gas law to solve for \( n \): \( n = \frac{PV}{RT} \).
Substitute the given values into the equation: \( P = 88 \text{ atm} \), \( V = 0.35 \text{ L} \), \( R = 0.0821 \text{ L atm K}^{-1} \text{ mol}^{-1} \), and \( T = 299 \text{ K} \).
Calculate the number of moles of helium using the rearranged equation.
Convert the number of moles of helium to mass using the molar mass of helium (4.00 g/mol).
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