Liquid N2O3 is dark blue at low temperatures, but the color fades and becomes greenish at higher temperatures as the compound decomposes to NO and NO2. At 25 degree C, a value of Kp = 1.91 has been established for this decomposition. If 0236 moles of N2O3 are placed in a 1.52-L vessel at 25 degree C, calculate the equilibrium partial pressures of N2O3(g), NO2(g) and NO(g).
N2O3(g) ----> NO2(g) + NO(g)
Kp = pNO*pNO2 / pN2O3
INITIAL PRESSURE OF n2o3 = nRT/V = 0.236*0.0821*298/1.52
= 3.8 atm
at equilibrium
pN2O3 = 3.8-x
pNO = X
pNO2 = X
1.91 = X^2/(3.8-X)
X = 1.9
partial pressure of N2O3 = 3.8-1.9 = 1.9 atm
partial pressure of NO = 1.9 atm
partial pressure of NO2 = 1.9 atm
Liquid N2O3 is dark blue at low temperatures, but the color fades and becomes greenish at...
2. Liquid N203 is dark blue at low temperatures, but the color fades and becomes greenish at higher temperatures as the compound decomposes to NO and NO2. At 25°C, a value of Kp = 1.91 has been established for this decomposition. If 0.236 moles of N2O3 are placed in a 1.52 L vessel at 25°C. calculate the equilibrium pressures of N2O3(), NO(g), and NO2(2).
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