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Solved: The equilibrium constant Kc for the reaction Is

Chapter 14, Problem 43P

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QUESTION:

The equilibrium constant \(K_{c}\) for the reaction

\(H_{2}(g)+B r_{2}(g)\ \leftrightharpoons\ 2 H B r(g)\)

is \(2.18 \times 10^{6}\) at \(730^{\circ} \mathrm{C}\). Starting with 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of \(\mathrm{H}_{2}\), \(B r_{2}\), and HBr at equilibrium.

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QUESTION:

The equilibrium constant \(K_{c}\) for the reaction

\(H_{2}(g)+B r_{2}(g)\ \leftrightharpoons\ 2 H B r(g)\)

is \(2.18 \times 10^{6}\) at \(730^{\circ} \mathrm{C}\). Starting with 3.20 moles of HBr in a 12.0-L reaction vessel, calculate the concentrations of \(\mathrm{H}_{2}\), \(B r_{2}\), and HBr at equilibrium.

ANSWER:

Step 1 of 4

The given reaction is as follows;

                                               

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