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
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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I need help finding the value of X and also verifying after usinf the simplifying assumption to solve for x.
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)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbd446b52-8c58-4d2e-95c3-f01363988023%2Fd69328db-59f8-4ca6-b0e7-0a4f0eac0557%2Fsw3fu8t_processed.jpeg&w=3840&q=75)
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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