Be sure to answer all parts. Enter your answers in scientific notation. At a particular temperature, Kc = 6.7 × 102 for 2NO(g) + 2H2(g) ⇌ N2(g) + 2H2O(g) Calculate Kc for each of the following reactions:(a) NO(g) + H2(g)1/2 N2(g) + H2O(g)

(b) 2 N2(g) + 4 H2O(g)4 NO(g) + 4 H2(g)

At a particular temperature, the equilibrium constants for the following reaction is:

2NO(g) + 2H₂(g) ⇄ N₂(g) + 2H₂O(g)   Kc = 6.7x10²      

So, the equilibrium constants for the given reactions are:

a. NO(g) + H₂(g) ⇄ 1/2N₂(g) + H₂O(g)   Kc = 2.6x10

b. 2N₂(g) + 4H₂O(g) ⇄ 4NO(g) + 4H₂(g)    Kc = 2.2x10⁻⁶  

The first reaction is:

2NO(g) + 2H₂(g) ⇄ N₂(g) + 2H₂O(g)   (1)

The equilibrium constant of the above reaction is:

   (2)  

Now, let's find the equilibrium constant for the given reactions.

a) The reaction is:

NO(g) + H₂(g) ⇄ 1/2N₂(g) + H₂O(g)   (3)

So, the constant for the reaction (3) is:

  (4)

When comparing equations (2) and (4), we can see that:

So, the equilibrium constant of the reaction (3) is:

Hence, the equilibrium constant for reaction (3) is 2.6x10.

b) The given reaction is:

2N₂(g) + 4H₂O(g) ⇄ 4NO(g) + 4H₂(g)    (5)

And the equilibrium constant is:

  (6)

From equations (2) and (6), we have first:

and second:

Hence, the equilibrium constant of the reaction (5) is:

Therefore, the equilibrium constant for this reaction is 2.2x10⁻⁶.

You can learn more about equilibrium constants here:

I hope it helps you!                          

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