The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acid solutions is 2 Br– + H2O2 + 2 H+ → Br2 + 2 H2O ? = ?[H2O2][H+][Br−] If the concentration of H2O2 is increased by a factor of three, by what factor is the rate of consumption of Br– ions increased
The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acid solutions is 2 Br– + H2O2 + 2 H+ → Br2 + 2 H2O ? = ?[H2O2][H+][Br−] If the concentration of H2O2 is increased by a factor of three, by what factor is the rate of consumption of Br– ions increased
Chemistry for Engineering Students
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Chapter12: Chemical Equilibrium
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Problem 12.1PAE: Identify the first chemical step in the production of Portland cement. How is this reaction related...
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The stoichiometric equation for the oxidation of bromide ions by hydrogen peroxide in acid
solutions is
2 Br– + H2O2 + 2 H+ → Br2 + 2 H2O ? = ?[H2O2][H+][Br−]
If the concentration of H2O2 is increased by a factor of three, by what factor is the rate of
consumption of Br– ions increased?
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