The first order rate constant for the decomposition of ethyl iodide by the reaction C 2 H 5 I g - C 2 H 5g - HI g at 600 K is 1-60- 10 -5 S -1 Its energy of activation is 209 kJ-mol- Calculate the rate constant of the reaction at 700 K-

logk_2k_1 = E_a2.303 × R (1T_1 1T_2) log k_21.6 ×10^ 5 = 2090002.303 × 8.314 (1600 1700) k_2 = 6.36 ×10^ 3S^ 1 ...

You visited us 1 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Rate Constant

The first ord...

Question

The first order rate constant for the decomposition of ethyl iodide by the reaction $C_{2} H_{5} I_{(g)} \to C_{2} H_{5 (g)} + {H I}_{(g)}$ at $600 K$ is ${1.60 \times 10}^{- 5} S^{- 1}$ Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700 K.

Open in App

Solution

$l o g \frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303 \times R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$l o g \frac{k_{2}}{1.6 \times 10^{- 5}} = \frac{209000}{2.303 \times 8.314} (\frac{1}{600} - \frac{1}{700})$

$k_{2} = 6.36 \times 10^{- 3} S^{- 1}$

Suggest Corrections

Similar questions

The first order rate constant for the decomposition of ethyl iodide by the reaction:

$C_{2} H_{5} I (g) \to C_{2} H_{4} (g) + H I (g)$

at $600 K$ is $1.60 \times 10^{- 5} s^{- 1}$ . Its energy of activation is $209 k J m o l^{- 1}$ . The rate constant of the reaction at $700 K$ will be:

Q. For a chemical reaction the specific rate constant at 600K is

1.60 \times 10^{6} s^{- 1}

, calculate the rate constant for the reaction at 700K, if energy of activation for the reaction is

2.209 K J {m o l}^{- 1}

Q. The decomposition of methyl iodide,

2 C H_{3} I (g) \to C_{2} H_{6} (g) + I_{2} (g)

, at

273^{o} C

has a rate constant of

2.418 \times 10^{- 5} s^{- 1}

. If activation energy for the reaction is

+ 179.9

k J

{m o l}^{- 1}

, what is the value of collision factor '

A

' at

273^{o} C

Q. A first order gas-phase reaction has an energy of activation of

240 k J m o l^{- 1}

. If the frequency factor of the reaction is

1. \times 10^{13} s^{- 1}

, calculate its rate constant at

600 K

Q. The energy of activation for a first order reaction is

104 k J m o l^{- 1}

. The rate constant at

25^{o} C

3.7 \times 10^{- 5} s^{- 1}

. What is the rate constant at

30^{o} C

Join BYJU'S Learning Program

The first order rate constant for the decomposition of ethyl iodide by the reaction C2H5I(g)→C2H5(g)+HI(g) at 600K is 1.60×10−5S−1 Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700 K.

logk2k1=Ea2.303×R(1T1−1T2)logk21.6×10−5=2090002.303×8.314(1600−1700)k2=6.36×10−3 S−1

The first order rate constant for the decomposition of ethyl iodide by the reaction $C_{2} H_{5} I_{(g)} \to C_{2} H_{5 (g)} + {H I}_{(g)}$ at $600 K$ is ${1.60 \times 10}^{- 5} S^{- 1}$ Its energy of activation is 209 kJ/mol. Calculate the rate constant of the reaction at 700 K.

$l o g \frac{k_{2}}{k_{1}} = \frac{E_{a}}{2.303 \times R} (\frac{1}{T_{1}} - \frac{1}{T_{2}})$

$l o g \frac{k_{2}}{1.6 \times 10^{- 5}} = \frac{209000}{2.303 \times 8.314} (\frac{1}{600} - \frac{1}{700})$

$k_{2} = 6.36 \times 10^{- 3} S^{- 1}$