1.

The reaction, "SO"_(2)"Cl"_(2)overset(k_(1))to"SO"_(2)+"Cl"_(2), is a first order reaction with k_(1)=2.2xx10^(-5)"sec"^(-1) at 575 K. What percentage of "SO"_(2)"Cl"_(2) will get decomposed in 90 minutes when the reaction is carried out at 575 K ?

Answer»

Solution :Since the REACTION is of the FIRST order (given), `k=(2.303)/(t)LOG""(a)/(a-x)`
Here, we are given that `k=2.2xx10^(-5)"SEC"^(-1)"",""t=90" MINUTES "=90xx60=5400" sec".`
`:.2.2xx10^(-5)s^(-1)=(2.303)/(5400s)log""(a)/(a-x)" or "log""(a)/(a-x)=0.0516" or "(a)/(a-x)="antilog "(0.0516)=1.127.`
or `""a=1.127a-1.127x" or "0.127a=1.127x`
`:.""(x)/(a)=(0.127)/(1.127)=0.113" or "%" decomposed "=0.113xx100=11.3%.`


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