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If $K_1$ and $K_2$ are respective equilibrium constants for the two reactions
$XeF_6 (g) + H_2O (g)  \rightleftharpoons  XeOF_4 (g) + 2HF (g)$
$XeO_4 (g) + XeF_6 (g) \rightleftharpoons XeOF_4 (g) + XeO_3F_2 (g)$
the equilibrium constant for the reaction $XeO_4 (g) + 2HF (g) \rightleftharpoons XeO_3F_2 (g) + H_2O (g)$ will be

• A
  $\frac{{{K_1}}}{{K_2^2}}$
• B
  $K_1K_2$
• C
  $\frac{{{K_1}}}{{{K_2}}}$
• ✓
  $\frac{{{K_2}}}{{{K_1}}}$