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in an experiment, 1.0 mol of N2O4 isplaced in a 10.0 L vessel and is allowed to react as describedbelow.

N2O4 (g) <==> 2 NO2(g)Kc= 4.0 * 10-7

Calculate the concentration of each species at equilibrium.

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Tod Thiel
Tod ThielLv2
28 Sep 2019

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Related questions

When 0.500 mol of N2O4 is placed in a 4.00 L reaction vessel and heated to 400 K, 79.3% of the N2O4 decomposes to NO2: N2O4 <------> 2 NO2

a) What is the molarity of N2O4 at equilibrium?

b) What is the molarity of NO2 at equilibrium?

c) Calculate Kc for the reaction.

d) Calculate Kp for the reaction.

1) The reaction 2 NO2 (g) >>> N2O4(g)
is studied at 298 K. Initially, 0.401 mol NO2 is placed in an empty1.0-L flask. At
equilibrium, the concentration of N2O4 is 0.184 mol/L. Calculate Kcfor the reaction.

2) Hydrogen and iodine react to form hydrogen iodide.

H2(g) + I 2 (g) 2 HI(g)
Kc is 0.504 at 25 °C. If initial concentrations of 0.170 M H2 and0.170 M I2 are allowed to equilibrate, what is the equilibriumconcentration of HI?

Thank you!

Calculate the equilibrium concentrations of N2O4 and NO2 at 25 ?C in a vessel that contains an initial N2O4 concentration of 0.0399M . The equilibrium constant Kc for the reaction N2O4(g)?2NO2(g) is 4.64

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