NUMBER 3 ONLY The equilibrium constant K, for the oxidation of sulfur dioxide into sulfur trioxide is 5.6×10s of BRF,, Br,, and F, at 250°C are 0.046 M, 1.2 M,2.Consider the given reaction.2BRF,Ce) = Br,(8) + 5F,(g)If the respective equilibrium concand 0.93 M, what are the values of K and Kponcentrations3.respectively, what is the partial pressure of O, in the system?2S0,(g) + 0,(g) = 2SO,(g)

Given-> Kp = 5.6 × 10^4 Peq.(SO2) = 0.64 atm Peq.(SO3)= 0.58 atm

Answered: The equilibrium constant K for the…

The equilibrium constant K for the ovidarion of sulfur dioxide 3. is 5.6x1 respectively, what is the partial pressure of O, in the system?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 50P

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Question

NUMBER 3 ONLY

The equilibrium constant K, for the oxidation of sulfur dioxide into sulfur trioxide is 5.6×10
s of BRF,, Br,, and F, at 250°C are 0.046 M, 1.2 M,
2.
Consider the given reaction.
2BRF,Ce) = Br,(8) + 5F,(g)
If the respective equilibrium conc
and 0.93 M, what are the values of K and Kp
oncentrations
3.
respectively, what is the partial pressure of O, in the system?
2S0,(g) + 0,(g) = 2SO,(g)

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