The reaction of nitrogen gas with oxygen gas, shown here, has a K_p value of 0.25. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.250 atm, what would be the equilibrium partial pressure of NO(g) ?
N₂(g) + O₂(g) 2NO(g)

Question

The reaction of nitrogen gas with oxygen gas, shown here, has a K_p value of 0.25. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.250 atm, what would be the equilibrium partial pressure of NO(g) ?
N₂(g) + O₂(g)

The reaction of nitrogen gas with oxygen gas, shown here, has a K<sub>p</sub> value of 0.25. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.250 atm, what would be the equilibrium partial pressure of NO(g) ? N<sub>2</sub>(g) + O<sub>2</sub>(g) 2NO(g) A) 0.100 atm B) 0.125 atm C) 0.166 atm D) 0.228 atm E) 0.351 atm

2NO(g)

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The Answer of The reaction of nitrogen gas with oxygen gas, shown here, has a K_p value of 0.25. If a closed vessel was charged with the two reactants, each at an initial partial pressure of 0.250 atm, what would be the equilibrium partial pressure of NO(g)? N₂(g) + O₂(g) 2NO(g)

The Reaction of Nitrogen Gas with Oxygen Gas, Shown Here