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WITCHER [35]
3 years ago
8

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?
Chemistry
1 answer:
sattari [20]3 years ago
7 0

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).

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