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

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

Step-by-step 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 * 10^(-3)`

when temperature 2,500 K the value of KP =
`3.6 * 10^(-3)`

value of kp=?

`KP= ((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).