At 25°c the decomposition of n2o5 (g) into no2 (g) and o2(g) follows first-order kinetics with k = 3.4×10−5 s−1. how long will it take for a sample originally containing 2.0 atm of n2o5 to reach a partial pressure of 380 torr?

11 hours

Explanation:

Half life: [A] = 1/2 [A]o

ln 1/2[A]o divided by ln [A]o = -kt

ln 1/2 = -kt

kt = - ln 1/2

t = 0.693/k

t = 0.693/ 3.4x10-5 s-¹

t1/2 = 20382,35s

20382,35s x 1h /3600s = 5,66 hours to 1 atm

380 torr equals to = 0.05 atm

5.66 x 2 = 11. 32 hours

the molecules move in straight line until they collide with each other or with the walls of the container. collisions are perfectly elastic; when two molecules collide, they change their directions and kinetic energies, but the total kinetic energy is conserved.

explanation:

catya that's not even a b or c