Question

The atmospheric oxidation of NO:

$\boxed{\sf \: 2NO(g)+O _2(g) \rightleftharpoons2NO _ 2(g)}$
$\rm \: was \: studied \: with \: initial \: \\ \rm pressure \: of \: 1 \: atm \: of \: \mathrm{NO } \: and \: 1 \\ \rm atm \: of \: \mathrm{O}_{2}. \: At \: equilibrium \: \\ \rm partial \: pressure \: of \: oxygen \: is \\ \rm 0.52atm \: calculate \: \mathrm{K}_{p} \: of \: the \: \\ \rm \: reaction.$
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Answer 1

Answer:

Answer is = 2

Explanation:

A + B - C

kp = (kp C ) / (kp A ) × (kp B )

o2 - initial pressure 0.5 atm

No - initial pressure 0.5 atm

No2 - initial pressure 0.5 -----for partial pressure - Xgas = nA /n Total × pressure total