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Chapter 14, Problem 28P(choose chapter or problem)
A 2.50-mole quantity of NOCI was initially in a 1.50-L reaction chamber at \(400^{\circ} \mathrm{C}\). After equilibrium was established, it was found that 28.0 percent of the NOCI had dissociated:
\(2 \mathrm{NOCl}(g)\ \leftrightharpoons\ 2 N O(g)+\mathrm{Cl}_{2}(g)\)
Calculate the equilibrium constant \(K_{C}\) for the reaction.
Questions & Answers
QUESTION:
A 2.50-mole quantity of NOCI was initially in a 1.50-L reaction chamber at \(400^{\circ} \mathrm{C}\). After equilibrium was established, it was found that 28.0 percent of the NOCI had dissociated:
\(2 \mathrm{NOCl}(g)\ \leftrightharpoons\ 2 N O(g)+\mathrm{Cl}_{2}(g)\)
Calculate the equilibrium constant \(K_{C}\) for the reaction.
ANSWER:Step 1 of 3
Dissociation of NOCl is given as;
We can determine the molarity of NOCl as follows:
