The decomposition of methyl iodide- 2C H 3 I g - C 2 H 6 g - I 2 g - at 273 o C has a rate constant of 2-418- 10 -5 s -1- If activation energy for the reaction is -179-9 kJ mol -1- what is the value of collision factor - A- at 273 o C-

log( 2.418× 10 ^ 5 ) =logA 179.9× 1000 2.303× 8.314× 546 log( 2.418× 10 ^ 5 ) + 179.9× 1000 2.303× 8.314× 546 =logA 4.616+17.208=logA ...

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Standard XII

Chemistry

Arrhenius Equation

The decomposi...

Question

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 $273^{o} C$ ?

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Solution

$l o g (2.418 \times 10^{- 5}) = l o g A - \frac{179.9 \times 1000}{2.303 \times 8.314 \times 546}$

$l o g (2.418 \times 10^{- 5}) + \frac{179.9 \times 1000}{2.303 \times 8.314 \times 546} = l o g A$

$- 4.616 + 17.208 = l o g A$

$A = 3.90 \times 10^{12} s^{- 1}$

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The decomposition of methyl iodide, 2CH3I(g)→C2H6(g)+I2(g), at 273oC has a rate constant of 2.418×10−5 s−1. If activation energy for the reaction is +179.9 kJ mol−1, what is the value of collision factor 'A' at 273oC?

log(2.418×10−5)=logA−179.9×10002.303×8.314×546log(2.418×10−5)+179.9×10002.303×8.314×546=logA−4.616+17.208=logAA=3.90×1012s−1

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 $273^{o} C$ ?

$l o g (2.418 \times 10^{- 5}) = l o g A - \frac{179.9 \times 1000}{2.303 \times 8.314 \times 546}$

$l o g (2.418 \times 10^{- 5}) + \frac{179.9 \times 1000}{2.303 \times 8.314 \times 546} = l o g A$

$- 4.616 + 17.208 = l o g A$

$A = 3.90 \times 10^{12} s^{- 1}$