Given the Following Equilibrium Equations Calculate K for the Decomposition of Dinitrogen Tetraoxide to Nitrogen

Given the following equilibrium equations, $\begin{array}{ll}2 \mathrm{~N}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{~N}_{2}(g) +\mathrm{O}_{2}(g) & K_{1}=8.3 \times 10^{34} \\\mathrm{~N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{NO}_{2}(g) & K_{2}=4.6 \times 10^{3} \\2 \mathrm{NO}_{2}(g) \rightleftharpoons \mathrm{N}_{2}(\mathrm{~g}) +2 \mathrm{O}_{2}(g) & K_{3}=5.9 \times 10^{16}\end{array}$
Calculate K for the decomposition of dinitrogen tetraoxide to nitrogen dioxide and oxygen.
$2 \mathrm{~N}_{2} \mathrm{O}_{4}(g) \rightleftharpoons 2 \mathrm{~N}_{2} \mathrm{O}(g) +3 \mathrm{O}_{2}(g)$ $\quad$ $\quad$ $\quad$ $K_{4}=?$

A) 1.1 × 10−⁴¹
B) 1.3 × 10−²⁰
C) 8.9 × 10−⁷
D) 3.3 × 10²¹
E) 2.3 × 10⁴⁹