At 500 k, the half-life period of a gaseous reaction at an initial pressure of 80 kPa is 350 s. when the pressure is 40 kPa, the half-life period is 175 s. The order of the reaction is

Question

Dr. Abubacker · Accepted Answer

(a)
$p_{1} = 80\ kPa\ ,\ \left( t_{1/2} \right)_{1} = 350s$
$p_{1} = 40\ kPa\ ,\ \left( t_{1/2} \right)_{1} = 175s$
$\frac{80}{40} = \frac{350}{175} = 2$
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$\because\frac{p_{1}}{p_{2}} = \frac{\left( t_{1/2} \right)_{1}}{\left( t_{1/2} \right)_{2}} = \frac{a_{1}}{a_{2}}$
$\left( t_{1/2} \right) \propto a(zero\ order\ reaction)$

Q. At 500 k, the half-life period of a gaseous reaction at an initial pressure of 80 kPa is 350 s. when the pressure is 40 kPa, the half-life period is 175 s. The order of the reaction is

Explanation

Reviewed by Dr. Abubacker

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