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If the reaction below has a Kp =1.9 × 106 at 400°C, what is Kc?
N2O(g) + NO2(g) 3NO(g)

A.
2.9 × 104
B.
5.3 × 106
C.
0.016
D.
0.16

Respuesta :

Answer : The value of [tex]K_c[/tex] is [tex]3.4\times 10^{4}[/tex]

Explanation :

The balanced equilibrium reaction is,

[tex]N_2O(g)+NO_2(g)\rightleftharpoons 3NO(g)[/tex]

The relation between [tex]K_p[/tex] and [tex]K_c[/tex] are :

[tex]K_p=K_c\times (RT)^{\Delta n}[/tex]

where,

[tex]K_p[/tex] = equilibrium constant at constant pressure = [tex]1.9\times 10^6[/tex]

[tex]K_c[/tex] = equilibrium concentration constant = ?

R = gas constant = 0.0821 L⋅atm/(K⋅mol)

T = temperature = [tex]400^oC=273+400=673K[/tex]

[tex]\Delta n[/tex] = change in the number of moles of gas = [(3) - (1 + 1)] = 1  (from the chemical reaction)

Now put all the given values in the above relation, we get:

[tex](1.9\times 10^6)=K_c\times (0.0821L.atm/K.mol\times 673K)^{1}[/tex]

[tex]K_c=3.4\times 10^{4}[/tex]

Thus, the value of [tex]K_c[/tex] is [tex]3.4\times 10^{4}[/tex]

tiffanyzheng1712

Answer:

A. 2.9 x 10^4

NOTE: When I did the calculations, I got the same amount as the person above so the answers in this question might be wrong.

Explanation:

Kp = 1.9 x 10^6, written in standard form: 1,900,000. Since the pressure is high (k < 1), the reaction favors the products so C. and D. are wrong.

Now it is either A. or B.

Kp, which is 1,900,000, is the total calculated pressure of the partial pressures of the reaction. That means B. 5.3 x 10^6, written out as 5,300,000 cannot be the Kc because it exceeds Kp = 1,900,000.

Also, Kp and Kc (partial pressure and concentration), are proportional to each other.

Therefore the answer is A. 2.9 x 10^4.

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