If \[{{K}_{1}}\] and \[{{K}_{2}}\] are respective equilibrium constants for the two reactions \[Xe{{F}_{6}}(g)+{{H}_{2}}O(g)\rightleftharpoons XeO{{F}_{4}}(g)+2HF(g)\] \[Xe{{O}_{4}}(g)+Xe{{F}_{6}}(g)\rightleftharpoons XeO{{F}_{4}}(g)+Xe{{O}_{3}}{{F}_{2}}(g)\] the equilibrium constant for the reaction \[Xe{{O}_{4}}(g)+2HF(g)\rightleftharpoons Xe{{O}_{3}}{{F}_{2}}(g)+{{H}_{2}}O(g)\] will be

• A. \[\frac{{{K}_{1}}}{K_{2}^{2}}\]                                
• B. \[{{K}_{1}}.{{K}_{2}}\]
• C. \[\frac{{{K}_{1}}}{{{K}_{2}}}\]                                  
• D. \[\frac{{{K}_{2}}}{{{K}_{1}}}\]