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3. The chemical reaction represented by the following balanced chemical equation takes place in aqueous solution: MnO4 + 5 Fe2 + 8 H → Mn2 + 5 Fe3 + 4 H2O When the disappearance of the permanganate ion, MnO4, is monitored, the rate of reaction for the consumption of the ion is 4.0x10 ² mol/L.s. Calculate the reaction rate for all other reactants and products.

3. The chemical reaction represented by the following balanced chemical equation takes place in aqueous solution: MnO4 + 5 Fe2 + 8 H → Mn2 + 5 Fe3 + 4 H2O When the disappearance of the permanganate ion, MnO4, is monitored, the rate of reaction for the consumption of the ion is 4.0x10 ² mol/L.s. Calculate the reaction rate for all other reactants and products.

Chemistry: Matter and Change
Chemistry: Matter and Change
1st Edition
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Chapter16: Reaction Rates
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Reaction rate calculation
3. The chemical reaction represented by the following balanced chemical equation takes place in aqueous solution: MnO4 + 5 Fe2 + 8 H → Mn2 + 5 Fe3 + 4 H2O When the disappearance of the permanganate ion, MnO4, is monitored, the rate of reaction for the consumption of the ion is 4.0x10 2 mol/L.s. Calculate the reaction rate for all other reactants and products.
Transcribed Image Text:3. The chemical reaction represented by the following balanced chemical equation takes place in aqueous solution: MnO4 + 5 Fe2 + 8 H → Mn2 + 5 Fe3 + 4 H2O When the disappearance of the permanganate ion, MnO4, is monitored, the rate of reaction for the consumption of the ion is 4.0x10 2 mol/L.s. Calculate the reaction rate for all other reactants and products.
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