The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g) 2NO(g)
At 2000°C, the equilibrium constant, K_c, has a value of 4.10 × 10^-4. What is the value of K_p?

Question

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g)

The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N<sub>2</sub>(g) + O<sub>2</sub>(g) 2NO(g) At 2000°C, the equilibrium constant, K<sub>c </sub>, has a value of 4.10 × 10<sup>-4</sup>. What is the value of K<sub>p</sub>? A) 2.17 × 10<sup>-8</sup> B) 4.10 × 10<sup>-4</sup> C) 7.65 × 10<sup>-2</sup> D) 7.75 E) none of the above

2NO(g)
At 2000°C, the equilibrium constant, K_c, has a value of 4.10 × 10^-4. What is the value of K_p?

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The Answer of The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N₂(g) + O₂(g) 2NO(g) At 2000°C, the equilibrium constant, K_c, has a value of 4.10 × 10^-4. What is the value of K_p?

The Reaction of Nitrogen with Oxygen to Form Nitrogen Monoxide