The Reaction Exhibits the Rate Law Where K $\times$

The reaction exhibits the rate law where k = 1.0 $\times$ 10^-5 M^-1 . s^-1 at 25°C.This reaction is run where the initial concentration of NOBr ([NOBr]₀) is 1.00 $\times$ 10^-1 M. The [NO] after 1.00 hour has passed is

A) 3.6 $\times$ 10^-4 M
B) 9.9 $\times$ 10^-3 M
C) 9.7 $\times$ 10^-3 M
D) 1.0 $\times$ 10^-3 M
E) none of these