For the following equilibrium,andrarr; Kp is found to be equal to Kc. This is attained when:a)0anddeg;Cb)273 Kc)1 Kd)12.18 KCorrect answer is option 'D'. Can you explain this answer?

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For the following equilibrium,

→

K_p is found to be equal to K_c. This is attained when:

a)
0°C
b)
273 K
c)
1 K
d)
12.18 K

Correct answer is option 'D'. Can you explain this answer?

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Verified Answer

For the following equilibrium,→ Kp is found to be equal to K...

Correct Answer: D (12.18 K)

Explanation:
The relationship between Kp and Kc is given by the equation:

Kp = Kc(RT)^(Δn)

where Δn is the change in the number of moles of gas in the reaction, R is the ideal gas constant, and T is the temperature in Kelvin.

For the given equilibrium, N2O4(g) → 2NO2(g), the change in the number of moles of gas, Δn, is:

Δn = (moles of products) - (moles of reactants)
Δn = 2 - 1
Δn = 1

We know that Kp = Kc, so:

Kc(RT)^(Δn) = Kc

This equation simplifies to:
RT = 1
Let's consider the possibility that the constant R used in the question is given in a different unit, such as atm·L/(mol·K). In this case, R = 0.0821 atm·L/(mol·K). We can solve for T again:

T = 1/R
T = 1/0.0821
T ≈ 12.18 K

This value matches option D, so the correct answer is 12.18 K.

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For the following equilibrium,→ Kp is found to be equal to K...

Kp= Kc (RT) ^delta ng

delta ng = 2-1 = 1
when Kp = Kc, Kp = Kp (RT) ^1
T = 1 / R = 1/ 0.0821 = 12.18

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