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An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature by the reaction


3H2(g) +N2(g) <=> 2NH3(g)

At equilibrium the concentrations are [H2]=5.0 M, [N2]= 8.0M, [NH3]=3.0M

What were the concentrations of nitrogen gas and hydrogen gas that were reacted initially.

Respuesta :

Answer: Concentrations of nitrogen gas and hydrogen gas that were reacted initially were 6.5 M and 0.5 respectively

Explanation:

Equilibrium constant is the ratio of the concentration of products to the concentration of reactants each term raised to its stochiometric coefficients.

      [tex]3H_2(g)+N_2(g)\rightarrow 2NH_3(g)[/tex]

at t= 0       x      y              0

tt t= eqm    (x-3z)   (y-z)      2z

2z = 3.0 M

z= 1.5 M

Initial concentration of [tex]H_2[/tex] = [tex]x-3\times z = 5.0 M[/tex]

[tex]x-3\times 1.5 =5.0M[/tex]

[tex]x=0.5M[/tex]

Initial concentration of [tex]N_2[/tex] = [tex]y-z =8.0M[/tex]

[tex]y-1.5=8.0M[/tex]

[tex]y=6.5M[/tex]

Thus concentrations of nitrogen gas and hydrogen gas that were reacted initially were 6.5 M and 0.5 respectively

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