The decomposition of N_(2)O_(5) in CCl_(4) solution follows the first order rate law. The concentrations of N_(2)O_(5) measured at different intervals are given below : {:("Time in seconds (t)",,,0,,,80,,,160,,,410,,,600,,,1130,,,1720),(["N"_(2)"O"_(5)]"mol"//"L",,,5.5,,,5.0,,,4.8,,,4.0,,,3.4,,,2.4,,,1.6):} Calculate the rate constant at t = 410 s and t = 1130 s. What do these results show ?

The decomposition of N_(2)O_(5) in CCl_(4) solution follows the first

1.	The decomposition of N_(2)O_(5) in CCl_(4) solution follows the first order rate law. The concentrations of N_(2)O_(5) measured at different intervals are given below : {:("Time in seconds (t)",,,0,,,80,,,160,,,410,,,600,,,1130,,,1720),(["N"_(2)"O"_(5)]"mol"//"L",,,5.5,,,5.0,,,4.8,,,4.0,,,3.4,,,2.4,,,1.6):} Calculate the rate constant at t = 410 s and t = 1130 s. What do these results show ?
Answer» SOLUTION :According to FIRST ORDER rate LAW, `K=(2.303)/(t)log""(a)/(a-x)=(2.303)/(t)log""(["N"_(2)"O"_(5)]_(0))/(["N"_(2)"O"_(5)]_(t))` `{:("At "t=410" s"",",,,k=(2.303)/(410s)log""(5.5)/(4.0)=7.768xx10^(-4)s^(-1)),("At "t=1130"s"",",,,k=(2.303)/(1130s)log""(5.5)/(2.4)=7.341xx10^(-4)s^(-1)):}` These results show that the rate constant is nearly constantat differenttimes.