Question

Consider this reaction: 2NH$_3$ (g) $\rightarrow$ N$_2$ (g) + 3H$_2$ (g) At a certain temperature it obeys this rate law. rate = (0.00191 s$^{-1}$) [NH$_3$] Suppose a vessel contains NH$_3$ at a concentration of 0.470M. Calculate how long it takes for the concentration of NH$_3$ to decrease to 17.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.

          Consider this reaction:
2NH$_3$ (g) $\rightarrow$ N$_2$ (g) + 3H$_2$ (g)
At a certain temperature it obeys this rate law.
rate = (0.00191 s$^{-1}$) [NH$_3$]
Suppose a vessel contains NH$_3$ at a concentration of 0.470M. Calculate how long it takes for the concentration of NH$_3$ to
decrease to 17.0% of its initial value. You may assume no other reaction is important.
Round your answer to 2 significant digits.

Consider this reaction:
2NH3 (g) → N2 (g) + 3H2 (g)
At a certain temperature it obeys this rate law.
rate = (0.00191 s^-1) [NH3]
Suppose a vessel contains NH3 at a concentration of 0.470M. Calculate how long it takes for the concentration of NH3 to
decrease to 17.0% of its initial value. You may assume no other reaction is important.
Round your answer to 2 significant digits.

Added by Debbie D.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

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O KINETICS AND EQUILIBRIUM Antonella Using first- and second-order integrated rate laws Consider this reaction: 2NH(g) -> N(g) + 3H2(g) At a certain temperature, it obeys this rate law: rate = (0.00191 s^(-1))[NH] Suppose a vessel contains NH at a concentration of 0.470 M. Calculate how long it takes for the concentration of NH to decrease to 17.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits.