Question

The following reaction follows zero order Kinetics



If the initial conc of W is  0.6M  and its  half life is 15 hours. When the initial conc of W is 1.5M, then time required to reach the final conc. of 0.6 M will be

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Answer 1

The half life if zero order rxn is given by

T=A/2k

A- initial concentration=0.6M

T=15 hours

K=0.6/30=0.02

A1=1.5

K=0.02

T1=A1/2k

T1=1.5/0.04

T1=37.5 hr

I hope this helps ( ╹▽╹ )

Answer 2

Answer:

The time required to reach the final concentration of 0.6M of W will be 45 hours.

Explanation:

Given: Initial conc. of W, ${[A_{o}]}=0.6M$

Half life of W, $t_{\frac{1}{2} }=15hours$

For zero order reaction,  $t_{\frac{1}{2} }=\frac{[A_{o}]}{2k}$

⇒   $k=\frac{[A_{o}]}{2t_{\frac{1}{2} }}$

Therefore rate constant, $k=\frac{0.6}{(2)(15)} =0.02Mhr^{-1}$

If  ${[A_{o}]}=1.5M$  and  ${[A_{t}]}=0.6M$ then time will be:

$t=\frac{[A_{o}]-{[A_{t}]}}{k}$

$t=\frac{1.5M-0.6M}{0.02Mhr^{-1}} =\frac{0.9M}{0.02Mhr^{-1}} =45hrs$

Therefore the concentration of W will be reduced from 1.5M to 0.6M after 45 hours.