A mixture of 5.17 mol N, and 24.14 g NO is heated in a closed vessel to 2000 °C. After heating, the total pressure of the mixture at equilibrium is 3.14 atm. N2(g) + O2(g) 2 NO(g) Kp = 0.101 at 2000°C In which direction does the reaction proceed after heating to 2000 °C? The reaction is at equilibrium. The reaction proceeds toward the products. The reaction proceeds toward the reactants. Calculate the equilibrium partial pressures of N2, O2, and NO at 2000 °C. PN2 = Po = atm atm

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A mixture of 5.17 mol N, and 24.14 g NO is heated in a closed vessel to 2000 °C. After heating, the total pressure of the
mixture at equilibrium is 3.14 atm.
N2(g) + O2(g) 2 NO(g)
Kp = 0.101 at 2000°C
In which direction does the reaction proceed after heating to 2000 °C?
The reaction is at equilibrium.
The reaction proceeds toward the products.
The reaction proceeds toward the reactants.
Calculate the equilibrium partial pressures of N2, O2, and NO at 2000 °C.
PN2
=
Po
=
atm
atm
Transcribed Image Text:A mixture of 5.17 mol N, and 24.14 g NO is heated in a closed vessel to 2000 °C. After heating, the total pressure of the mixture at equilibrium is 3.14 atm. N2(g) + O2(g) 2 NO(g) Kp = 0.101 at 2000°C In which direction does the reaction proceed after heating to 2000 °C? The reaction is at equilibrium. The reaction proceeds toward the products. The reaction proceeds toward the reactants. Calculate the equilibrium partial pressures of N2, O2, and NO at 2000 °C. PN2 = Po = atm atm
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