The reverse Haber reaction has a rate constant of 1.45×10-6 molarity times seconds inverse at 25°C. Now calculate the half life for the reaction where the initial concentration of ammonia equals 2.47×10-2 moles per liter.
Right. So here we know that this is a zeroth order reaction because remember for a 0th order reaction the units for your rate constants are molarity times time inverse. So the fact that it's molarity times seconds inverse tells us this is a 0 order reaction.
So here that means that half life equals the initial concentration of your reactant divided by 2K. So this becomes a simple plug and chug type of question. We have the initial concentration of R reactant in terms of ammonia divided by two times our rate constant, here molarity times seconds. Inverse the molarities will cancel out and our half life will be in seconds.
So this comes out to be 8.52×103 seconds. So this would be our final answer.