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Question

Chemistry Question on Equilibrium Constant

What is the equilibrium expression for the reaction, P4(s)+5O2(g)⇌P4O10(s)?{{P}_{4}}(s)+5{{O}_{2}}(g) \rightleftharpoons {{P}_{4}}{{O}_{10}}(s)?

A

Kc=[P4O10][P4][O2]5{{K}_{c}}=\frac{[{{P}_{4}}{{O}_{10}}]}{[{{P}_{4}}]{{[{{O}_{2}}]}^{5}}}

B

Kc=[P4O10]5[P4][O2]{{K}_{c}}=\frac{[{{P}_{4}}{{O}_{10}}]}{5[{{P}_{4}}][{{O}_{2}}]}

C

Kc=[O2]5{{K}_{c}}={{[{{O}_{2}}]}^{5}}

D

Kc=1[O2]5{{K}_{c}}=\frac{1}{{{[{{O}_{2}}]}^{5}}}

Answer

Kc=1[O2]5{{K}_{c}}=\frac{1}{{{[{{O}_{2}}]}^{5}}}

Explanation

Solution

In the expression for equilibrium constant ( Kp{{K}_{p}} or Kc{{K}_{c}} ) species in solid state are not written (ie, their molar concentrations are taken as
P4(s)+5O2⇌P4O10(s){{P}_{4}}(s)+5{{O}_{2}} \rightleftharpoons {{P}_{4}}{{O}_{10}}(s)
Thus, Kc=1[O2]5{{K}_{c}}=\frac{1}{{{[{{O}_{2}}]}^{5}}}