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The decomposition of "N"(2)"O"(5)(g), i....

The decomposition of `"N"_(2)"O"_(5)(g), i.e.,"N"_(2)"O"_(5)(g)to4"NO"_(2)(g)+"O"_(2)(g)` is a first order reaction with a rate constant of `5xx10^(-4)"sec"^(-1)" at "45^(@)C`. If intial concentration of `"N"_(2)"O"_(5)` is 0.25 M, calculate its concentration after 2 min. Also calculate half life for the decomposition of `"N"_(2)"O"_(5)(g).`

Text Solution

Verified by Experts

`k=5xx10^(-4)"sec"^(-1),a=0.25" M",(a-x)=?`
`t=2" min "=120" sec"`
For a first order reaction, `k=(2.303)/(t)log""(a)/(a-x):.5xx10^(-4)=(2.303)/(120)log""(0.25)/((a-x))" or "log""(0.25)/((a-x))=0.026`
`:." "(0.25)/(a-x)="Antilog "0.026=1.062" or "(a-x)=(0.25)/(1.062)M=0.235M`
`t_(1//2)=(0.693)/(k)=(0.693)/(5xx10^(-4)"sec"^(-1))=1386" sec"=23" min "6" sec".`
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With rate constant of 5 xx 10^(-4)sec^(-1) at 45^(@) C, If initial concentration of N_(2)O_(5) is 0.25 M, Calcualte the concentration after 2 minutes. Also calculate half life for the decomposition of N_(2)O_(5) ? 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g)

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