?At \(1285^{\circ} \mathrm{C}\), the equilibrium constant for the reaction
Chapter 15, Problem 15.47(choose chapter or problem)
At \(1285^{\circ} \mathrm{C}\), the equilibrium constant for the reaction \(\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{Br}(g)\) is \(K_{c}=1.04 \times 10^{-3}\). A 0.200-L vessel containing an equilibrium mixture of the gases has 0.245 g \(\mathrm{Br}_{2}(g)\) in it. What is the mass of Br(g) in the vessel?
Text Transcription:
1285^circ C
Br_2(g) \rightleftharpoons 2 (g)
K_c=1.04 \times 10^-3
Br_2(g)
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