Chapter 12, Problem 54QAP

Consider the following hypothetical reaction:

${\text{X}}_2\left(g\right)+\text{R}\left(s\right)\rightleftharpoons {\text{X}}_2\text{R}\left(g\right)$

R has a molar mass of 73 g/mol. When equilibrium is established, a 2.5-L reaction vessel at 125°C contains 15.0 g of R, 4.3 atm of X₂, and 0.98 atm of X₂R.

(a) Calculate K for the reaction at 125°C.

(b) The mass of R is doubled. What are the partial pressures of X₂ and X₂R when equilibrium is reestablished?

(c) The partial pressure of X₂ is decreased to 2.0 atm. What are the partial pressures of X₂ and X₂R when equilibrium is reestablished?