Consider a mixture of Argon and water vapor at $100$ C and $200$ kPa contained in a

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$10$ L insulated tank. Use appendix B for water and ideal gas law for Argon.

$($a$)$ If the water vapor is saturated, what is the partial pressure of water? $[1$ Pt$]$

$($b$)$ How many moles of Argon is in the tank? $[2$ Pts$]$

$($c$)$ What is the mass of Argon in the tank? $[1$ Pt$]$

$($d$)$ What are the mole fractions of the two components in the mixture? $[2$ Pts$]$

$($e$)$ What are the mass fractions of the two components in the mixture? $[2$ Pts$]$

$($f$)$ Can you solve this question with the concept of partial volume instead of partial pressure? Try predicting what the final state of water would be and see if it is consistent with the given conditions $[2$ Pts$].$

$($Note: $($f$)$ is purely conceptual, meaning you do not need calculations. We will get to the notion behind this question, in terms of $($why$)/($why not$),$ later in the course.$)$