Question

The decomposition of NO2(g) occurs by the following bimolecular elementary reaction. 2 NO2(g) → 2 NO(g)...

The decomposition of NO2(g) occurs by the following bimolecular elementary reaction.

2 NO2(g) → 2 NO(g) + O2(g)

The rate constant at 273 K is 2.3 ✕ 10-12 L/mol · s, and the activation energy is 111 kJ/mol. How long will it take for the concentration of NO2(g) to decrease from an initial partial pressure of 4.0 atm to 2.4 atm at 451 K? Assume ideal gas behavior.

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Answer #1

temperature T1 = 273 K

T2 = 451 K

rate constant k1 = 2.3 x 10^-12 /mol.s

activation energy = 111 kJ/mol

ln (k2 / k1) = Ea / R [1 / T1 - 1 / T2]

ln (k2 / 2.3 x 10^-12) = 111 / 8.314 x 10^-3 [1/273 - 1/ 451]

k2 = 5.55 x 10^-4 L/mol . s

rate constant at 451 K = 5.55 x 10^-4 L/mol . s

initial pressure = 4.0 atm

M = P / RT = 4.0 / 0.0821 x 273 = 0.178 M

concentration of NO2 = 0.1785 M

final concnetration = 2.4 / 0.0821 x 451 = 0.0648 M

k = 1/ t ln (Ao / At)

5.55 x10^-4 = 1 / t ln (0.1785 / 0.0648)

t = 1825 sec

time taken = 1825 sec

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