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Chemistry Question on Chemical Kinetics

For the reaction H++BrO3−+3Br−−>5Br+2+H2O{H^+ + BrO_3 ^- + 3Br^- -> 5Br+2 + H_2O} which of the following relation correctly represents the consumption & formation of reactants and products :

A

d[Br2]dt=−53d[Br−]dt\frac{d [Br_2]}{dt} =-\frac{5}{3} \frac{d [Br^-]}{dt}

B

d[Br2]dt=−d[Br−]dt\frac{d [Br_2]}{dt} =- \frac{d [Br^-]}{dt}

C

d[Br2]dt=35d[Br−]dt\frac{d [Br_2]}{dt} =\frac{3}{5} \frac{d [Br^-]}{dt}

D

d[Br2]dt=−35d[Br−]dt\frac{d [Br_2]}{dt} =-\frac{3}{5} \frac{d [Br^-]}{dt}

Answer

d[Br2]dt=−35d[Br−]dt\frac{d [Br_2]}{dt} =-\frac{3}{5} \frac{d [Br^-]}{dt}

Explanation

Solution

Rate of disappearance of reactant
\hspace20mm = Rate of appearance of prodcut
\hspace10mm -\frac{1}{5}\frac{d [Br^-]}{dt} =+\frac{1}{3} \frac{d [Br_2]}{dt}
or        d[Br2]dt=−35d[Br−]dt \, \, \, \, \, \, \, \frac{d [Br_2]}{dt}=-\frac{3}{5}\frac{d [Br^-]}{dt}