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One mole of each \( \mathrm{Cl}_{2}(\mathrm{~g}) \) and \( \mathrm{Br}_{2}(\mathrm{~g}) \) were taken in a \( 2 \mathrm{~L} \) flask, sealed and heated to some temperature where the following equilibrium was established and at equilibrium, the mole \( \% \) of \( \mathrm{ClBr}(\mathrm{g}) \) was \( 40 \% \).
\[
\mathrm{Cl}_{2}(\mathrm{~g})+\mathrm{Br}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{BrCl}(\mathrm{g})
\]
At equilibrium, 2 mol of \( \mathrm{NO} \) gas was added where the following additional equilibrium was established.
\[
2 \mathrm{NO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NOCl}(\mathrm{g})
\]
At new equilibrium, mixture was found to contain \( 0.9 \mathrm{~mol} \) of \( \operatorname{BrCl}(\mathrm{g}) \). Determine \( K_{C} \) for the two equilibria in Eq. (1) and (2).
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