Consider this reaction: 2Cl2O5 —> 2Cl2 + 5O2

At a certain temperature it obeys this rate law.
rate = (2.7.M^-1•s^-1) [Cl2O5]^2

Suppose a vessel contains Cl2O5 at a concentration of 0.600M. calculate how long it takes for the concentration of Cl2O5 to decrease by 94%. you may assume no other reaction is important. round your answer to two digits

Explanation:

Hello,

In this case, we have a second order kinetics given the second power of the concentration of chlorine (V) oxide in the rate expression, thus, the integrated equation for the concentration decay is:

Thus, the final concentration for a 94% decrease is:

Therefore, we compute the time for such decrease:

Regards.

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.