Consider the following reaction 2 N2O(g) → 2 N2(g) + O2(g) rate = k [N2O] . For an initial concentration of N2O of 0.50 M, calculate the concentration of N2O remaining after 2.0 min if k = 3.4 × 10−3 s −1 . 1. 0.17 M 2. 0.50 M 3. 0.55 M 4. 0.33 M 5. 0.66 M

0.33 M

Explanation:

As the order of the reaction is one, Expression for rate law for first order kinetics is given by:

where,

k = rate constant  =

t = age of sample  = 2.0 min =

a = let initial amount of the reactant  = 0.50 M

a - x = amount left after decay process  = ?

Now put all the given values in above equation, we get

Thus the concentration of remaining after 2.0 min is 0.33 M

i do not get it   at all

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.