?A mixture of 1.374 g of \(\mathrm{H}_{2}\) and 70.31 g of \(\mathrm{Br}_{2}\) is heated
Chapter 15, Problem 15.36(choose chapter or problem)
A mixture of 1.374 g of \(\mathrm{H}_{2}\) and 70.31 g of \(\mathrm{Br}_{2}\) is heated in a 2.00-L vessel at 700 K. These substances react according to
\(\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{HBr}(g)\)
At equilibrium, the vessel is found to contain 0.566 g of \(\mathrm{H}_{2}\).
(a) Calculate the equilibrium concentrations of \(\mathrm{H}_{2}, \mathrm{Br}_{2}\), and HBr.
(b) Calculate \(K_{c}\).
Text Transcription:
Br_2
H2(g) + Br2(g) \rightleftharpoons 2 HBr(g)
H_2
K_c
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