Part A Calculate the equilibrium constant for the formation of NO2 (g) from NO (g) and O2 (g) at 405 K. 2 NO (g) + O2 (g) → 2 NO2 (g) Calculate the equilibrium constant for the formation of NO2 (g) from NO (g) and O2 (g) at 405 K. 2 NO (g) + O2 (g) → 2 NO2 (g)
2 NO (g) + O2 (g) → 2 NO2 (g)
H = Hp -HR
= 2*33.2 -(2*90.2-0) = -114Kj/mole
S = S0p - S0R
= 2*240-(2*210.7+205) = -146.4J/mole-K = -0.1464Kj/mole-K
G0 = H -TS
= -114-298*-0.1464 = -70.3728KJ/mole
G0 = -RTlnK
-70372 = -8.314*405*298logK
logK = -70372/-1003416.66
logK = 0.07013
K = 100.07013 = 1.1752 >>>>>> answer
Part A Calculate the equilibrium constant for the formation of NO2 (g) from NO (g) and...
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