Given that K eq = 2.4*10³ for the reaction below at 2000 C and the initial partial pressure of NO equals 37.3 atm, what is the equilibrium partial pressure of NO at this temperature?
2 NO (g) N₂(g) + O₂(g)

Question

Given that K eq = 2.4*10³ for the reaction below at 2000 C and the initial partial pressure of NO equals 37.3 atm, what is the equilibrium partial pressure of NO at this temperature?
2 NO (g) Given that K eq = 2.4*10<sup>3</sup> for the reaction below at 2000 C and the initial partial pressure of NO equals 37.3 atm, what is the equilibrium partial pressure of NO at this temperature? 2 NO (g) N₂(g) + O₂(g) A) 0.37 atm B) 0.75 atm C) 18.5 atm D) 18.8 atm E) 37.3 atm

Given that K eq = 2.4*10<sup>3</sup> for the reaction below at 2000 C and the initial partial pressure of NO equals 37.3 atm, what is the equilibrium partial pressure of NO at this temperature? 2 NO (g) N₂(g) + O₂(g) A) 0.37 atm B) 0.75 atm C) 18.5 atm D) 18.8 atm E) 37.3 atm

N₂(g) + O₂(g)

Quizplus · Accepted Answer

The Answer of Given that K eq = 2.4*10³ for the reaction below at 2000 C and the initial partial pressure of NO equals 37.3 atm, what is the equilibrium partial pressure of NO at this temperature? 2 NO (g) N₂(g) + O₂(g)

Given That K Eq = 2