Question

hydrogen and oxygen gases are mixed in a 2.0 l container at 350 k. the hydrogen gas exerts a pressure of 1.4 atm, and the oxygen gas exerts a pressure of 0.24 atm. how many moles of oxygen are present in the mixture? 8.8 mols 60. mols 0.017 mols 0.11 mols

Explanation:

Step1: Use ideal gas law

The ideal gas law is \(PV = nRT\), where \(P\) is pressure, \(V\) is volume, \(n\) is the number of moles, \(R\) is the ideal gas constant (\(R=0.0821\space L\cdot atm/(mol\cdot K)\)), and \(T\) is temperature. We want to find \(n\) for oxygen. Given \(P = 0.24\space atm\), \(V=2.0\space L\), \(T = 350\space K\).

Step2: Rearrange the formula for \(n\)

Rearrange \(PV=nRT\) to \(n=\frac{PV}{RT}\).
Substitute the values: \(n=\frac{0.24\times2.0}{0.0821\times350}\)

$$
LATEXBLOCK0
$$

Answer:

0.017 mols