For the chemical equation SO,(g) + NO,(g)= SO, (g) + NO(g) the equilibrium constant at a certain temperature is 2.20. At this temperature, calculate the number of moles of NO, (g) that must be added to 3.12 mol SO,(g) in order to form 1.30 mol SO,(g) at equilibrium. 0.25 moles of NO,(g): mol Incorrect
For the chemical equation SO,(g) + NO,(g)= SO, (g) + NO(g) the equilibrium constant at a certain temperature is 2.20. At this temperature, calculate the number of moles of NO, (g) that must be added to 3.12 mol SO,(g) in order to form 1.30 mol SO,(g) at equilibrium. 0.25 moles of NO,(g): mol Incorrect
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 14.40QE
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it is also not 0.25
![For the chemical equation
SO, (g) + NO, (g)= SO, (g) + NO(g)
the equilibrium constant at a certain temperature is 2.20. At this temperature, calculate the number of moles of NO, (g) that must
be added to 3.12 mol SO, (g) in order to form 1.30 mol SO, (g) at equilibrium.
0.25
moles of NO,(g):
mol
Incorrect](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe5571744-3b39-46e3-aed6-0b0d5cfca8ba%2F3104f526-8781-453c-bca8-262289501725%2Fh8q3kx_processed.png&w=3840&q=75)
Transcribed Image Text:For the chemical equation
SO, (g) + NO, (g)= SO, (g) + NO(g)
the equilibrium constant at a certain temperature is 2.20. At this temperature, calculate the number of moles of NO, (g) that must
be added to 3.12 mol SO, (g) in order to form 1.30 mol SO, (g) at equilibrium.
0.25
moles of NO,(g):
mol
Incorrect
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