Consider this reaction: →2nh3g+n2g3h2g at a certain temperature it obeys this rate law: rate =2.11·m−1s−1nh32 suppose a vessel contains nh3 at a concentration of 0.590m. calculate how long it takes for the concentration of nh3 to decrease by 88.0%. you may assume no other reaction is important. round your answer to 2 significant digits

5.9 s

Explanation:

Let's consider the following reaction.

2 NH₃(g) ⇄ N₂(g) + 3 H₂(g)

The rate law is:

rate = 2.11 M⁻¹s⁻¹[NH₃]²

where

2.11 M⁻¹s⁻¹ is the rate constant (k)

2 is the order of reaction for NH₃

The initial concentration of NH₃ ([NH₃]₀) is 0.590 M. If it decreases by 88.0%, the final concentration ([NH₃]) will be 100.0% - 88.0% = 12.0% of the initial concentration, that is, 0.0708 M.

For a second order reaction we can use the following expression.

it's all four options.