The equilibrium constant for the following reaction will be P4(s) +5O2(g) leftharpoons P4O10(s)

Question

The equilibrium constant for the following reaction will be P4(s) +5O2(g) leftharpoons P4O10(s) (A) Kc=([P4][O2]5/[P4O10]) (B) Kc=(1/[O2]5) (C) Kc=([P4O10]/[P4][O2]5) (D) Kc=[O2]5

Tardigrade Admin · Accepted Answer

P4(s) +5O2(g)leftharpoons P4O10(s) Since concentration of solids is taken as 1, expression for equilibrium constant involves only oxygen. Kc=(1/[O2]5)

Q. The equilibrium constant for the following reaction will be
$P_{4 (s)} + 5 O_{2 (g)} ⇌ P_{4} O_{10 (s)}$

$K_{c} = \frac{[ P _{4} ] [ O _{2} ] ^{5}}{[ P _{4} O _{10} ]}$

$K_{c} = \frac{1}{[ O _{2} ] ^{5}}$

$K_{c} = \frac{[ P _{4} O _{10} ]}{[ P _{4} ] [ O _{2} ] ^{5}}$

$K_{c} = [O_{2}]^{5}$

$P_{4 (s)} + 5 O_{2 (g)} ⇌ P_{4} O_{10 (s)}$
Since concentration of solids is taken as $1$ , expression for equilibrium constant involves only oxygen.
$K_{c} = \frac{1}{[ O _{2} ] ^{5}}$

Q. The equilibrium constant for the following reaction will be P4(s)​+5O2(g)​⇌P4​O10(s)​

Kc​=[P4​O10​][P4​][O2​]5​

Kc​=[O2​]51​

Kc​=[P4​][O2​]5[P4​O10​]​

Kc​=[O2​]5