The reaction below is carried out at a different temperature at which Kc = 0.055. This time, however, the reaction mixture starts with only the product, [NO] = 0.0100 M, and no reactants. Find the equilibrium concentrations of N₂, O2, and NO at equilibrium. N₂(g) + O₂(g) = 2NO(g) Express your answers to three significant figures separated by commas.
The reaction below is carried out at a different temperature at which Kc = 0.055. This time, however, the reaction mixture starts with only the product, [NO] = 0.0100 M, and no reactants. Find the equilibrium concentrations of N₂, O2, and NO at equilibrium. N₂(g) + O₂(g) = 2NO(g) Express your answers to three significant figures separated by commas.
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 13Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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N2=
O2=
NO=
i got x=18.201 and that was incorrect, thanks for the help
![The reaction below is carried out at a different temperature at which Kc = 0.055. This time,
however, the reaction mixture starts with only the product, [NO] = 0.0100 M, and no
reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium.
N₂(g) + O₂(g) = 2NO(g)
Express your answers to three significant figures separated by commas.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3d57ba8c-0b2f-4dbb-833e-9f04fd4157c5%2Fb3dae46f-50c0-4345-a5ae-e8981e7ceb2e%2F7j8xx1j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The reaction below is carried out at a different temperature at which Kc = 0.055. This time,
however, the reaction mixture starts with only the product, [NO] = 0.0100 M, and no
reactants. Find the equilibrium concentrations of N2, O2, and NO at equilibrium.
N₂(g) + O₂(g) = 2NO(g)
Express your answers to three significant figures separated by commas.
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