Recall that the unit for the rate constant is given by:

$\overline{){\mathbf{k}}{\mathbf{=}}{{\mathbf{M}}}^{\mathbf{n}\mathbf{-}\mathbf{1}}{\mathbf{\xb7}}{{\mathbf{s}}}^{\mathbf{-}\mathbf{1}}}$

The given rate constant only has **s ^{–1}** as its units, which means

The ** integrated rate law** for a first-order reaction is as follows:

$\overline{){\mathbf{ln}}{{\mathbf{\left[}}{\mathbf{A}}{\mathbf{\right]}}}_{{\mathbf{t}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{kt}}{\mathbf{+}}{\mathbf{ln}}{{\mathbf{\left[}}{\mathbf{A}}{\mathbf{\right]}}}_{{\mathbf{0}}}}$

For the decomposition of gaseous dinitrogen pentoxide,

2N_{2}O_{5}(*g*) ⟶ 4NO_{2}(*g*) + O_{2}(*g*)

the rate constant is *k* = 2.8 x 10^{-3} s^{-1} at 60°C. The initial concentration of N_{2}O_{5} is 1.58 mol/L.

(a) What is [N_{2}O_{5}] after 5.00 min?

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.