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For the reaction I₂(g) 2 I(g) the value of K = 3.76 x 10-5 at 1000 K. If 1.00 moles of I₂ is placed into a 2.00 L flask and heated, what will be the equilibrium concentrations of [1₂] and [I]? (Hint: you will need to use the quadratic formula to solve for x)

For the reaction I₂(g) 2 I(g) the value of K = 3.76 x 10-5 at 1000 K. If 1.00 moles of I₂ is placed into a 2.00 L flask and heated, what will be the equilibrium concentrations of [1₂] and [I]? (Hint: you will need to use the quadratic formula to solve for x)

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.34PAE: 1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was...
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I need help finding the value of X and also verifying after usinf the simplifying assumption to solve for x.

When checking if the assumption is valid for the reaction on the slide, the % obtained was: between 3.0% and 4.0% between 0.0% and 0.60 % between 4.0% and 5.0% between 2.0% and 3.0% between 1.5% and 2.0% between 1.0 % and 1.5% between 0.60% and 1.0%
Transcribed Image Text:When checking if the assumption is valid for the reaction on the slide, the % obtained was: between 3.0% and 4.0% between 0.0% and 0.60 % between 4.0% and 5.0% between 2.0% and 3.0% between 1.5% and 2.0% between 1.0 % and 1.5% between 0.60% and 1.0%
For the reaction I₂(g) 2 I(g) the value of K. = 3.76 x 10-5 at 1000 K. If 1.00 moles of I2 is placed into a 2.00 L flask and heated, what will be the equilibrium concentrations of [1₂] and [I]? (Hint: you will need to use the quadratic formula to solve for x)
Transcribed Image Text:For the reaction I₂(g) 2 I(g) the value of K. = 3.76 x 10-5 at 1000 K. If 1.00 moles of I2 is placed into a 2.00 L flask and heated, what will be the equilibrium concentrations of [1₂] and [I]? (Hint: you will need to use the quadratic formula to solve for x)
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