Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of : 0.0067·Ms−1: 2N2O(g)→2N2(g)+O2(g)
Suppose a flask is charged under these conditions with of ammonia. After how much time is there only left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to significant digits.

Explanation:

From the given information:

The above reaction is a zero-order reaction.

The rate constant = 0.0067 M-s⁻¹

Suppose the volume of the flask = 4L

Initial Mol of dinitrogen monoxide = 300 mmol

The final mol of dinitrogen monoxide = 150 mmol

The molarity of dinitrogen monoxide =

= 0.0075 mmol/L

= 0.0075 L

The final concentration  

= 0.0375 L

By applying zero order equation

the electrical  conductivity  of asolution  of an electrolyte is measured by determining the resistance of thesolution  between two flat or cylindrical electrodes separated by a fixed distance.

wher is the rest of the question