Answer to Question #64924 in Inorganic Chemistry for sanjeet

Question #64924
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).
Expert's answer
N2O3 = NO2 + NO

First, the mol of each component can be calculated from the equation [NO2][NO]/[N2O3] = Kp. Thus, C(N2O3) = 0.026 mol, C(NO2) = 0.210 mol and C(NO) = 0.210 mol.
According to a perfect gas state equation p = n*R*T/V. Thus, p(N2O3) = 42.4 kPa, p(NO2) = 342 kPa and p(NO) = 342 kPa.

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!


No comments. Be the first!

Leave a comment

New on Blog