The rate constant for decomposition of COCl2g according to following reaction COCl2g - COg - Cl2 g- - H - 19 kcal-mol- expressed as ln k - 15 - 5000TCalculate activation energy for given reaction- in K cal-mol-

ln k = 15 5000T ln k ln(3.27 ×10^6) = 5000T ln k3.27 ×10^6 = 5000T k = 3.27×10^6×e^ 10/RT Here the activation energy is 10 K cal/ ...

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Activation Energy

The rate cons...

Question

The rate constant for decomposition of $C O C l_{2} (g)$ according to following reaction $C O C l_{2} (g) \to C O (g) + C l_{2} (g); Δ H = 19 k c a l / m o l$ , expressed as $l n k = 15 - \frac{5000}{T}$
Calculate activation energy for given reaction. $(i n K c a l / m o l)$ .

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C O (g) + C l_{2} (g) ⇋ C O C l_{2} (g)

K_{p} / K_{c}

C O (g) + C l_{2} (g) ⇌ C O C l_{2} (g)

\frac{K_{p}}{K_{c}}

{C O}_{(g)} + {C l}_{2 (g)} ⇌ {C O C l}_{2 (g)}

K_{p} / K_{c}

C O_{(g)} + C l_{2 (g)} ⇋ C O C l_{2 (g)}

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C O {C l}_{2} (g) ⇌ C O (g) + {C l}_{2} (g); K_{1} = 0.329

2 C O (g) + O_{2} (g) ⇌ 2 C O_{2} (g); K_{2} = 2.24 \times 10^{22}

1000 K

2 C O {C l}_{2} (g) + O_{2} (g) ⇌ 2 C O_{2} (g) + {C l}_{2} (g)

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