A chemist mixes 0.120 M Br2 and 0.150 M Cl₂ in a flask at 250 °C. The compounds react according to the equation below. Br2 (g) + Cl2 (g) 2 BrCl (g) °C Kea The concentration at equilibrium for the Br2 is and BrCl is 23.8 at 250

Chemistry: Principles and Practice
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Chapter14: Chemical Equilibrium
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Problem 14.52QE: Consider 0.200 mol phosphorus pentachloride sealed in a 2.0-L container at 620 K. The equilibrium...
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A chemist mixes 0.120 M Br₂ and 0.150 M Cl₂ in a flask at
250 °C. The compounds react according to the equation
below.
Br2 (g) + Cl2 (g)
2 BrCl
(g)
°C
Kea
The concentration at equilibrium for the Br2 is
and BrCl is
23.8 at 250
Transcribed Image Text:A chemist mixes 0.120 M Br₂ and 0.150 M Cl₂ in a flask at 250 °C. The compounds react according to the equation below. Br2 (g) + Cl2 (g) 2 BrCl (g) °C Kea The concentration at equilibrium for the Br2 is and BrCl is 23.8 at 250
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