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For the reaction N2 (g) + O2 (g) 2NO (g), theKeq at 2130°C is 0.0025.

Assume [N2] = 0.95 M, [O2] = 0.65 M, and[NO] = 0.050 M.

Calculate Q and describe the direction thereaction will shift

Respuesta :

kenmyna
   N2  + O2  = 2No
The Q  value  of the  above equation is  calculated as   below

Q =[ No]^2/{(O2)(N2)}

Q=[0.05]^2/{(0.95 )(0.65)} = 0.00404

the reaction will shift to the left  since  Q> Keq that is  0.0404 > 0.0025

Answer: The value of Q is 0.004 and reaction will shift towards the right.

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as [tex]K_{eq}[/tex]

K is the constant of a certain reaction when it is in equilibrium, while Q is the quotient of activities of products and reactants at any stage other than equilibrium of a reaction.

For the given chemical reaction:

[tex]N_2(g)+O_2(g)\rightarrow 2NO(g)[/tex]

The expression for [tex]Q[/tex] is written as:

[tex]Q=\frac{[NO]^2}{[N_2]^1[O_2]^1}[/tex]

[tex]Q=\frac{[0.050]^2}{[0.95]^1[0.65]^1}[/tex]

[tex]Q=0.004[/tex]

Given :  [tex]K_{eq}[/tex] = 0.0025

Thus as [tex]K_{eq}<Q[/tex], the reaction will shift towards the right i.e. towards the product side.

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