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earnstyle [38]
3 years ago
15

Ethyl chloride vapor decomposes by the first-order reaction C2H5Cl → C2H4 + HCl The activation energy is 249 kJ/mol and the freq

uency factor is 1.60 × 1014 s−1. Find the value of the specific rate constant at 896 K . Enter your answer numerically (to 4 decimal places) and in terms of the appropriate units for a first order reaction.
Chemistry
1 answer:
maw [93]3 years ago
7 0

Answer : The value of rate constant is, 0.3607s^{-1}

Explanation :

The Arrhenius equation is written as:

K=A\times e^{\frac{-Ea}{RT}}

Taking logarithm on both the sides, we get:

\ln k=-\frac{Ea}{RT}+\ln A             ............(1)

where,

k = rate constant

Ea = activation energy  = 249 kJ/mol = 249000 kJ/mol

T = temperature  = 896 K

R = gas constant  = 8.314 J/K.mole

A = pre-exponential factor  or frequency factor = 1.60\times 10^{14}s^{-1}

Now we have to calculate the value of rate constant by putting the given values in equation 1, we get:

\ln k=-\frac{249000J/mol}{8.314J/K.mol\times 896K}+\ln (1.60\times 10^{14}s^{-1})

\ln k=-1.0198

k=0.3607s^{-1}

Therefore, the value of rate constant is, 0.3607s^{-1}

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