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Consider the reaction. Upper n subscript 2 (g) plus 3 upper H subscript 2 (g) double-headed arrow 2 upper N upper H subscript 3 (g). At equilibrium, the concentrations of the different species are as follows. [NH3] = 0.105 M [N2] = 1.1 M [H2] = 1.50 M What is the equilibrium constant for the reaction at this temperature? 0.0030 0.030 34 340

Respuesta :

Answer:

A

Explanation:

Eduard22sly

The equilibrium constant for the reaction at the given temperature given the data is 0.003

What is equilibrium constant?

The equilibrium constant for a given reaction is the ratio of the concentration of the products raised to their coefficients to the concentration of the reactants raised to their coefficients.

nA + eB <=> cD + xE

The equilibrium constant for the above reaction is given as

Keq = [D]^c × [E]^x / [A]^n × [B]^e

How to determine the equilibrium constant

  • N₂ + 3H₂ <=> 2NH₃
  • Concentration of nitrogen [N₂] = 1.1 M
  • Concentration of Hydrogen [H₂] = 1.5 M
  • Concentration of ammonia [NH₃] = 0.105 M
  • Equilibrium constant (Keq) =?

Keq = [NH₃]² / [N₂] × [H₂]³

Keq = (0.105)² / [1.1 × (1.5)³]

Keq = 0.003

Learn more about equilibrium constant:

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