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 rate of reaction will remain the same, because k will decrease by half. 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.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 rate of reaction will remain the same, because k will decrease by half. 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.