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Practice problem 9.4

the equilibrium constant for the system at this temperature?

6.4 x 10 mol/dm³ of N2, 1.7 x 10 mol/dm³ of O2 and 1.1 *10^ - mol/dm³ of NO. What is

An equilibrium mixture of N_{2} U_{2} and NO gases at 1500K is determined to consist of

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Eduard22sly

The equilibrium constant for the system at the given temperature is 1.1×10⁻⁵

What is equilibrium constant?

Equilibrium constant for a given is defined as the concentration of the products raised to their coefficient to the concentration of the reactants raised to their coefficient

For example:

eB <=> cD

The equilibrium constant for the reaction above is given as

Ke = [D]^c / [B]^e

How to determine the equilibrium constant

  • N₂(g) + O₂(g) <=> 2NO(g)
  • [N₂] = 6.4×10⁻³ M
  • [O₂] = 1.7×10⁻³ M
  • [NO] = 1.1×10⁻⁵ M
  • Equilibrium constant (Ke) =?

The equilibrium constant for the reaction reaction can be obtained as follow

Ke = [NO]² / [N₂][O₂]

Ke = [1.1×10⁻⁵]² / [6.4×10⁻³][1.7×10⁻³]

Ke = 1.1×10⁻⁵

Thus, the equilibrium constant for the reaction at the given temperature is 1.1×10⁻⁵

Learn more about equilibrium constant:

https://brainly.com/question/17960050

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