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A first order gas reaction has k = 1.5 x...

A first order gas reaction has `k = 1.5 xx 10^(-6) s^(-1)` at `200^(@)C`. If the reaction is allowed to run for `10 h`, what have changed in the Product? What is the half-life of this reaction?

Text Solution

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`t=2.303/K "log" N_(0)/N`
Given: `K=1.5xx10^(-6) sec^(-1)` (thus reaction is I order), `t=10 hour`
`10xx60xx60=2.303/(1.5xx10^(-6)) "log" N_(0)/N`
`:. N_(0)/N=1.0555`
`:. N=0.9475xxN_(0)`
`:.` Product formed `=N_(0)-0.9475 N_(0)`
`=0.0525 N_(0)=5.25%`
Also `t_(1//2)=0.693/K=0.693/(1.5xx10^(-6)`
`=462000 sec =128.33 hr`
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