## Chemistry and Chemical Reactivity (9th Edition)

a) Since doubling H2O2 concentration doubles the initial rate, the reaction is of first-order: $r=k[H_2O_2]$ b) In the first line: $5.3\times10^{-5}\ mol/L.min=k\times0.05\ mol/L$ $k=0.00106\ min^{-1}$ c) Previously $r=\Delta[O_2]/\Delta t$, now $r'=-\Delta[H_2O_2]/\Delta t=-2\dot{}\Delta[O_2]/\Delta t=2\dot{}r$ therefore: $k'=2\dot{}k$