Consider the reaction: 2NO¿(g) +7H2(g) = 2NH3(g) + 4H20(1) a) Write the expression for the equilibrium constant for the above balanced reaction. b) In a 1.0 L sealed container, 6.021 moles of NO2 and 3.908 moles of H2 are combined. The reaction proceeds until equilibrium is reached at 1800 K, at which point there are 0.825 moles of NH3 present. Determine the equilibrium constant for this reaction. c) In a different 1.0 L reaction vessel at 1800 K, 3.66 moles of NO2, 0.75 moles of H2, 3.53 moles of NH3, and 8.22 moles of H2O are present. Is this reaction at equilibrium? If it is not, which direction is the reaction proceeding in?

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b and c please

5) Consider the reaction:
2NO2(g) + 7H2(g) = 2NH3(g) + 4H20(I)
a) Write the expression for the equilibrium constant for the above balanced
reaction.
b) In a 1.0 L sealed container, 6.021 moles of NO2 and 3.908 moles of H2 are
combined. The reaction proceeds until equilibrium is reached at 1800 K, at which
point there are 0.825 moles of NH3 present. Determine the equilibrium constant for
this reaction.
c) In a different 1.0 L reaction vessel at 1800 K, 3.66 moles of NO2, 0.75
moles of H2, 3.53 moles of NH3, and 8.22 moles of H20 are present. Is this reaction at
equilibrium? If it is not, which direction is the reaction proceeding in?
Transcribed Image Text:5) Consider the reaction: 2NO2(g) + 7H2(g) = 2NH3(g) + 4H20(I) a) Write the expression for the equilibrium constant for the above balanced reaction. b) In a 1.0 L sealed container, 6.021 moles of NO2 and 3.908 moles of H2 are combined. The reaction proceeds until equilibrium is reached at 1800 K, at which point there are 0.825 moles of NH3 present. Determine the equilibrium constant for this reaction. c) In a different 1.0 L reaction vessel at 1800 K, 3.66 moles of NO2, 0.75 moles of H2, 3.53 moles of NH3, and 8.22 moles of H20 are present. Is this reaction at equilibrium? If it is not, which direction is the reaction proceeding in?
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