The reaction 2NO(g) + Br₂ (g) — 2 NOBr(g) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br2 is 0.0250 atm and the equilibrium partial pressure of NOBr is 0.0857 atm, calculate the partial pressure of NO at equilibrium. Partial pressure = atm

The reaction 2NO(g) + Br₂ (g) — 2 NOBr(g) has Kp = 109 at 25°C. If the equilibrium partial pressure of Br2 is 0.0250 atm and the equilibrium partial pressure of NOBr is 0.0857 atm, calculate the partial pressure of NO at equilibrium. Partial pressure = atm

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 30P

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Question

The reaction
2 NO(g) + Br₂ (g) — 2 NOBr(g)
has K₂ = 109 at 25°C. If the equilibrium partial pressure of Br2 is 0.0250 atm and the equilibrium partial pressure of NOBr is 0.0857 atm,
calculate the partial pressure of NO at equilibrium.
Partial pressure =
atm

An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction
3 H₂(g) + N2(g) → 2 NH3(g)
At equilibrium, the concentrations are [H₂] = 6.0 M, [N₂] = 12 M, and [NH3] = 4.0 M. What were the concentrations of nitrogen gas and
hydrogen gas that were reacted initially?
[H₂]0=
[N2]0=
M
> >
M

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