Consider the inter conversion of nitrosotriacetoamine into nitrogen phorone and water. The reaction is 1st order in each direction, with an equilibrium constant of 104, the activation energy for the forward reaction is 57.45 kj / mol. Assuming arrehenius preexponetial factor of 1012 s

Consider the inter conversion of nitrosotriacetoamine into nitrogen phorone and water.

The reaction is 1st order in each direction, with an equilibrium constant of 10⁴, the activation energy for the forward reaction is 57.45 kj / mol. Assuming arrehenius preexponetial factor of 10¹² s^–1.6

Linked Question 1

If the change in entropy of the reaction is 0.07 KJ. K^–1mol^–1 at 1 atm pressure. Calculate up to which temperature the reaction would not be spontaneous. (For forward reaction)

T > 250 K

T < 285.7 K

T > 200 K

T < 340.2 K

ΔG = ΔH – TΔS

ΔG = 20 – T x 0.07

For non-spontaneous process ΔG > 0

hence 0 < 20 – T x 0.07

T < $\frac{20}{0.07}$ ⇒ T < 285.7 K

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Linked Question 2

What is the expected forward constant at 300K, it we initiate this reaction starting with only reactant

10⁶

10⁸

10²

10⁴

log Kb = $\log A - \frac{Ea}{2.303 RT}$

log Kb = $12 - \frac{57450}{2.303 \times 8.314 \times 300}$

Log Kb = 2

Kb = Antilog 2

Kb = 102

Kc = $\frac{K_{F}}{K_{b}}$ ⇒ 104 = $\frac{K_{F}}{10^{2}}$

KF = 106

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Linked Question 3

Calculate Kp of the reaction at 300K

10⁴atm

24.6 × 10⁴atm

2.4 × 10⁴ atm^–1

2.82 × 10² atm^–1

K_p = K_c(RT)^Δn

= 10⁴ (0.082 x 300)¹

= 24.6 x 10⁴

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