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Exhibit 14-4 Consider the Reaction Below and Its Corresponding Equilibrium

question 156

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Exhibit 14-4 Consider the reaction below and its corresponding equilibrium constant at 2000 C to answer the following question(s) :
N₂(g) + O₂(g) Exhibit 14-4 Consider the reaction below and its corresponding equilibrium constant at 2000 C to answer the following question(s) : N₂(g)  + O₂(g)    2 NO (g)  K c = 4.10 10 - 4 (at 2000 C)  Complete the table shown below for an experiment where 0.35 moles of N₂is mixed with 0.15 moles of O₂in a 1.00 liter reaction vessel and the reaction mixture is allowed to come to equilibrium. Concentration N₂O₂ 2 NO Initial 0.35 M 0.15 M Change At equilibrium -Refer to Exhibit 14-4. What equilibrium expression shown below would allow you to solve for x and therefore enable you to solve for the equilibrium concentrations of each of the substances present at equilibrium? A)  4x<sup>2</sup>/(0.35 + x) (0.15 + x)  = 4.1×10<sup> - 4</sup> B)  4x<sup>2</sup>/(0.35 - x) (0.15 - x)  = 4.1×10<sup> - 4</sup> C)  2x<sup>2</sup>/(0.35 - x) (0.15 - x)  = 4.1×10<sup> - 4</sup> D)  x<sup>2</sup>/(0.35 - x) (0.15 - x)  = 4.1×10<sup> - 4</sup> E)  2x<sup>2</sup>/(0.35 + x) (0.15 + x)  = 4.1×10<sup> - 4</sup> 2 NO (g) K c = 4.10 10 - 4 (at 2000 C)
Complete the table shown below for an experiment where 0.35 moles of N₂is mixed with 0.15 moles of O₂in a 1.00 liter reaction vessel and the reaction mixture is allowed to come to equilibrium. Concentration N₂O₂ 2 NO Initial 0.35 M 0.15 M Change At equilibrium
-Refer to Exhibit 14-4. What equilibrium expression shown below would allow you to solve for x and therefore enable you to solve for the equilibrium concentrations of each of the substances present at equilibrium?


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