Question

In: Chemistry

The decomposition of CCl3CHS can be considered to be the following. (1) CH3CHS  CH3 +...

The decomposition of CCl3CHS can be considered to be the following. (1) CH3CHS  CH3 + CHS (2) CH3 + CH3CHS  CH4 + CH3CS (3) CH3CS  CS + CH3 (4) 2CH3  C2H6 The CHS reacts to form very minor amounts of other moeities. (i) Determine the initiation, propagation and termination steps. (ii) Determine the overall reaction neglecting the minor species cited. (iii) Determine r for the reaction where k = k2(k1/2k4)1/2.

Expert Solution

The reactions are

(i)

CH3CHS --> CH3 + CHS.......(initiation) (let rate constant =K1]

CH3 + CH3CHS --> CH4 + CH3CS ............(propagation) (rate constant = K2)

CH3CS --> CS + CH3............(propagation) (rate constant = K3)

2CH3 --> C2H6..........(termination) (rate constant = K4)

(ii) 2CH3CHS --> C2H6 + H2S (overall reaction)

(iii) Rate of reaction = d[C2H6] / dt = K4[CH3]^2 ......(1)

Applying Steady state approximation to CH3

d[CH3 ] / dt = 0 = K1[CH3CHS] - K2[CH3][CH3CHS] + K3 [CH3CS] - 2K4[CH3]^2 ...(2)

Applying SSA to CH3CS

d[CH3CS ] / dt = 0 = K2[CH3][CH3CHS] -K3 [CH3CS] = 0 ....................(3)

Add (2) and (3)

K1[CH3CHS] - 2K4[CH3]^2 = 0

So [CH3]^2 = K1[CH3CHS] / 2K4

[CH3] = (K1[CH3CHS] / 2K4)^1/2 ...............(4)

Rate of reaction = d[C2H6] / dt = K4[CH3]^2 (Put 4 in this)

Rate of reaction = d[C2H6] / dt = K4 K1 [CH3CHS] / 2

K1K4 / 2 = K

Rate of reaction = K [CH3CHS]

queen_honey_blossom answered 3 years ago

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