If for a hypothetical reaction,E_a = 0 at 273 | vedclass

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(B) The Arrhenius equation is given by $k = A e^{-\frac{E_a}{RT}}$.Given that the activation energy $E_a = 0$.Substituting $E_a = 0$ into the equation

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(B) The Arrhenius equation is given by $k = A e^{-\frac{E_a}{RT}}$.Given that the activation energy $E_a = 0$.Substituting $E_a = 0$ into the equation,we get $k = A e^0 = A 	imes 1 = A$.Since the rate constant $k$ becomes independent of temperature $T$ when $E_a = 0$,the rate constant at any temperature will be equal to the frequency factor $A$.Therefore,$k_{383 \ K} = A$ and $k_{273 \ K} = A$.The ratio of the rate constants is $\frac{k_{383 \ K}}{k_{273 \ K}} = \frac{A}{A} = 1$.

$Case$	$E_a \ (kcal/mol)$	$Temp. \ Change \ (K)$
$I$	$40$	$200 - 210$
$II$	$80$	$200 - 210$
$III$	$40$	$300 - 310$
$IV$	$80$	$300 - 310$

If for a hypothetical reaction,$E_a = 0$ at $273 \ K$,then find the ratio of the rate constants at $383 \ K$ and $273 \ K$.

Similar Questions

Write the Arrhenius equation representing the relationship between the rate constants $k_1$ and $k_2$ at two different temperatures $T_1$ and $T_2$.

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$Case$ $E_a \ (kcal/mol)$ $Temp. \ Change \ (K)$
$I$ $40$ $200 - 210$
$II$ $80$ $200 - 210$
$III$ $40$ $300 - 310$
$IV$ $80$ $300 - 310$

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