Consider the equilibrium between dinitrogen tetroxide and nitrogen dioxide:

$N_2{O}_4(g)2N{O}_2(g),K_p=0\mathrm{.}660at319K$

$($a$)$ What is the value of $K_c$ for this reaction? $($b$)$ What is the value of $K_p$ for the reaction $2N{O}_2(g)N_2{O}_4(g)?($c$)$ If the equilibrium partial pressure of $N{O}_2(g)$ is $0\mathrm{.}332$atm, what is the equilibrium partial pressure of $N_2{O}_4(g)?$