Answer:
[tex]\large \boxed{\text{2.35 atm}}[/tex]
Explanation:
We can use Dalton's Law of Partial Pressures:
Each gas in a mixture of gases exerts its pressure independently of the other gases
[tex]\begin{array}{rcl}p_{\text{He}} + p_{\text{Ar}}+ p_{\text{Xe}} &= & p_{\text{tot}} \\\text{0.300 atm} + \text{0.350 atm} + p_{\text{Xe}}& = &\text{3.00 atm}\\\text{0.650 atm}+ p_{\text{Xe}}& = &\text{3.00 atm}\\p_{\text{Xe}} & = &\text{3.00 atm - 0.650 atm} \\& = & \textbf{2.35 atm}\\\end{array}\\\text{The partial pressure of xenon is $\large \boxed{\textbf{2.35 atm}}$}[/tex]
