Iodine, I2, and bromine, Br2, react to produce iodine monobromide, IBr. I₂(g) + Br₂ (g) ⇒ 2IBr(g) A starting mixture of 0.5000 mol I2 and 0.5000 mol Br₂ reacts at 150°C to produce 0.4221 mol IBr at equilibrium. What would be the equilibrium composition (in moles) of a mixture that starts with 6.860 mol I2 and 6.040 mol Br₂? n(1₂) = n(Br₂) n(IBr) = = = mol mol mol
Iodine, I2, and bromine, Br2, react to produce iodine monobromide, IBr. I₂(g) + Br₂ (g) ⇒ 2IBr(g) A starting mixture of 0.5000 mol I2 and 0.5000 mol Br₂ reacts at 150°C to produce 0.4221 mol IBr at equilibrium. What would be the equilibrium composition (in moles) of a mixture that starts with 6.860 mol I2 and 6.040 mol Br₂? n(1₂) = n(Br₂) n(IBr) = = = mol mol mol
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:Iodine,
I2, and bromine,
Br2, react to produce iodine monobromide,
IBr.
I2(g) + Br₂(g) →⇒ 2IBr(g)
A starting mixture of 0.5000 mol
I2 and 0.5000 mol
Br₂ reacts at 150°C to produce 0.4221 mol
IBr at equilibrium. What would be the equilibrium
composition (in moles) of a mixture that starts with 6.860
mol
I2 and 6.040 mol
Br₂?
n(I₂) =
n(Br₂)
n(IBr):
=
=
=
mol
mol
mol
Transcribed Image Text:The major constituents of the atmosphere are nitrogen,
N2, and oxygen,
O₂. Dry atmospheric air at a pressure of 1.000 atm has a
partial pressure of
N₂ of 0.781 atm and a partial pressure of
O2 of 0.209 atm. At high temperatures,
N₂ and
O₂ react to produce nitrogen monoxide (nitric oxide),
NO.
N₂(g) + O₂(g) → 2NO(g)
Suppose a sample of dry air is raised to 2153°C in a hot
flame and then rapidly cooled to fix the amount of
NO formed. If
K₂ for this reaction at this temperature is
2.8 × 10-³, how many grams of
NO would be produced from 194.0 g of dry air?
g
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