S2O82−(aq)+3I−(aq)→2SO42−(aq)+I3−(aq) In aqueous solution, the reaction represented by the balanced equation shown above has the experimentally determined rate law: rate=k[S2O82−][I−]. If the concentration of [S2O82−] is doubled while keeping [I−] constant, which of the following experimental results is predicted based on the rate law, and why?
S2O82−(aq)+3I−(aq)→2SO42−(aq)+I3−(aq)
In aqueous solution, the reaction represented by the balanced equation shown above has the experimentally determined rate law: rate=k[S2O82−][I−].
If the concentration of [S2O82−] is doubled while keeping [I−] constant, which of the following experimental results is predicted based on the rate law, and why?
A The
B The rate of reaction will double, because the rate is directly proportional to [S2O82−]..
C The rate of reaction will increase by a factor of four, because two moles of SO42− are produced for each mole of S2O82− consumed.
D The rate of reaction will increase by a factor of four, because the reaction is second order overall.
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