?The equilibrium \(2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2
Chapter 15, Problem 15.33(choose chapter or problem)
The equilibrium \(2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{NOCl}(g)\) is established at 500 K. An equilibrium mixture of the three gases has partial pressures of 0.095 atm, 0.171 atm, and 0.28 atm for NO, \(\mathrm{Cl}_{2}\), and NOCl, respectively.
(a) Calculate \(K_{p}\) for this reaction at 500.0 K.
(b) If the vessel has a volume of 5.00 L, calculate \(K_{c}\) at this temperature.
Text Transcription:
2 NO(g) + Cl_2(g) \rightleftharpoons 2 NOCl(g)
Cl_2
K_p
K_c
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