At a given temperature, the equilibrium constant (Kp) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.154. If 0.198 atm N2O4 is sealed in a flask, what partial pressure (in atm) of NO2 will exist at equilibrium?N2O4(g) ⇄ 2NO2(g)(no scientific notation)

Answered: At a given temperature, the equilibrium…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section: Chapter Questions

Problem 8PS: An equilibrium mixture of SO2, O2, and SO3 at a high temperature contains the gases at the following...

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At a given temperature, the equilibrium constant (K_p) for the decomposition of dinitrogen tetraoxide to nitrogen dioxide is 0.154. If 0.198 atm N₂O₄ is sealed in a flask, what partial pressure (in atm) of NO₂ will exist at equilibrium?
N₂O₄(g) ⇄ 2NO₂(g)

(no scientific notation)

Expert Solution

Introduction

In equilibrium concepts, it is quite common to come across various equilibrium constants. The equilibrium constant (K) becomes quite helpful while expressing the relationship between products and reactants for a particular reaction (under equilibrium conditions).

Given data:

The equilibrium constant K_p is 0.154.

Initial pressure of N₂O₄ is 0.198 atm.

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