N2(g) + O2(g) ⇌ 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and PO2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of Kp?
N2(g) + O2(g) ⇌ 2NO(g) If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and PO2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of Kp?
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 116IP: Given K = 3.50 at 45C for the reaction A(g)+B(g)C(g) and K = 7.10 at 45C for the reaction...
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N2(g) + O2(g) ⇌ 2NO(g)
If N2(g) and O2(g) are placed in a flask at a constant temperature with the initial pressures of PN2 = 0.78 atm and PO2 = 0.21 atm, the equilibrium pressure of NO(g) that forms is PNO = 1.7 x 10-2 atm. What is the value of Kp?
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