The decomposition of N_(2)O_(5)(g) is a first order reaction with a rate constant of 5xx10^(-4)s^(-1) at 45^(@)C. i.e., 2N_(2)O_(5)(g) to 4NO_(2)(g)+O_(2)(g). If initial concentrationof N_(2)O_(5) is 0.25M, calculate its concentration after 2 min. Also calculate half-life for decomposition of N_(2)O_(5) (g).

The decomposition of N_(2)O_(5)(g) is a first order reaction with a ra

1.	The decomposition of N_(2)O_(5)(g) is a first order reaction with a rate constant of 5xx10^(-4)s^(-1) at 45^(@)C. i.e., 2N_(2)O_(5)(g) to 4NO_(2)(g)+O_(2)(g). If initial concentrationof N_(2)O_(5) is 0.25M, calculate its concentration after 2 min. Also calculate half-life for decomposition of N_(2)O_(5) (g).
Answer» SOLUTION :`k=5xx10^(-4)s^(-1), [R]_(0)=0.25 M, t=2 "min"=120S` USING `k=(2.303)/(t)"log"([R]_(0))/([R])" or log"([R]_(0))/([R])=(kt)/(2.303)` Substituting the values, we GET `"log"(0.25)/([R])=(5xx10^(-4)xx120)/(2.303)=0.02605 or (0.25)/([R])=` ANTILOG 0.02605 = 1.061 or`[R]=(0.25)/(1.061)=0.23M` `t_(1//2)=(0.693)/(k)=(0.693)/(5xx10^(-4)) or t_(1//2)=1386`