We’re being asked to determine the time it will take for 26.0% of the initial amount of ^{96}Nb to be consumed.

Recall that ** radioactive/nuclear decay of isotopes** follows

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

where:

**[N] _{t}** = concentration at time t

The nuclide ^{96}Nb decays by a first-order process with a rate constant of 2.96×10^{–2} min^{-1}. How long will it take for 26.0% of the initial amount of ^{96}Nb to be consumed?

A) 44.0 h

B) 0.170 h

C) 27.7 h

D) 6.70 h

E) 0.758 h

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