Question

The equilibrium constants for the chemical reaction N 2(g) + O 2(g) 2NO(g) are K P = 1.1 × 10 –3 and 3.6 × 10 –3 at 2,200 K and 2,500 K, respectively. Which one of these statements is true?

Answer 1

Answer:

The answer is "At 2200K, NO(g)'s partial pressure is below 2500K. C.KP by a factor of (RT) is lower than Kc"

Explanation:

In the given question choices were missing so, the correct choice can be defined as follows:

Given:

Reaction equation: $\bold{N_2(g) + O_2(g) \longrightarrow 2NO(g)}$

when temperature 2,200 K the value of KP = $1.1 \times 10^{-3}$

when temperature 2,500 K the value of KP = $3.6 \times 10^{-3}$

value of kp=?

$KP= \frac{(PNO)^2}{(PN_2)(PO_2)}$

In the above formula the value of $(PN_2) and (PO_2)$ is defined in the denominator section and the value of $(PNO)$ is defined in the numerator section that defines the value of KP is increases.so, the temperature of the KP will be KP ∝ (PNO).