Nitrogen pentoxide decomposes according to equation 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) The first order reaction was allowed to proceed at 140^(@)C and the data below were collected. a) Calculate rate constant in all the cases. b) What will be the concentration of N_(2)O_(5) after 100 minutes? c) Calculate initial rate of reaction.

Nitrogen pentoxide decomposes according to equation 2N_(2)O_(5)(g) to

1.	Nitrogen pentoxide decomposes according to equation 2N_(2)O_(5)(g) to 4NO_(2)(g) + O_(2)(g) The first order reaction was allowed to proceed at 140^(@)C and the data below were collected. a) Calculate rate constant in all the cases. b) What will be the concentration of N_(2)O_(5) after 100 minutes? c) Calculate initial rate of reaction.
Answer» SOLUTION :a) For FIRST order reaction , k`=(2.303)/tloga/(a-x)` In first CASE `k=2.303/(20 min)log(0.400)/0.289 = 2.303/(20 min)log400/289 = 2.303/(20 min)[log 400 - log 289]` `=2.303/(20 min) [2.6201 - 2.4609]=(2.303 xx 0.1412)/(20 mm) = 1.63 xx 10^(-2) min^(-1)` In second case `k=2.303/(40 min) log 0.400/0.209 = 2.303/(40 min) log 400/209 = 2.303/(40 min)[log 400- log 209]` `=2.303/(40 min) [2.6021 - 2.3201] = (2.303 xx 0.2820)/(40 min)= 1.62 xx 10^(-1) min^(-1)` In third case