H2O2(aq) + 2I-(aq) + 2H3O+(aq) → I2(aq) + 4H2O(l) (Reaction 1) I2(aq) + 2S2O32-(aq) → S4O62-(aq) + 2I-(aq) (Reaction 2) I2(aq) + I-(aq) + Starch(aq) → (I3- -Starch)complex (aq) (Reaction 3) Now consider the moment when the blue colour change is about to occur (i.e. when there is no more thiosulfate remaining in solution).Based on the initial experiment and initial concentrations of reagents, calculate the concentrations of the reagents present in the flask at the moment just before the blue colour change begins (ignore the starch, and the S4O62- which is formed as the other by-product in this reaction).Does Reaction (1) continue beyond this point? Multiple choice 2 Question 10a. yesb. no Based on what you have calculated, which reagent in Reaction (1) is the limiting reagent?Multiple choice 3 Question 10a. H+b. H2O2c. I-d. S2O32-
Question
H2O2(aq) + 2I-(aq) + 2H3O+(aq) → I2(aq) + 4H2O(l) (Reaction 1) I2(aq) + 2S2O32-(aq) → S4O62-(aq) + 2I-(aq) (Reaction 2) I2(aq) + I-(aq) + Starch(aq) → (I3- -Starch)complex (aq) (Reaction 3) Now consider the moment when the blue colour change is about to occur (i.e. when there is no more thiosulfate remaining in solution).Based on the initial experiment and initial concentrations of reagents, calculate the concentrations of the reagents present in the flask at the moment just before the blue colour change begins (ignore the starch, and the S4O62- which is formed as the other by-product in this reaction).Does Reaction (1) continue beyond this point? Multiple choice 2 Question 10a. yesb. no Based on what you have calculated, which reagent in Reaction (1) is the limiting reagent?Multiple choice 3 Question 10a. H+b. H2O2c. I-d. S2O32-
Solution
The text you provided is a chemistry problem, but it's missing some crucial information needed to solve it, such as the initial concentrations of the reagents. However, I can still provide some general guidance.
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To determine the concentrations of the reagents just before the blue color change, you would need to know the stoichiometry of the reactions and the initial concentrations. You would then use the stoichiometry to calculate how much of each reagent is consumed or produced.
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Whether Reaction (1) continues beyond this point depends on whether there are still reactants left. If there is still H2O2 and I- remaining, then the reaction can continue. However, if either of these is used up (i.e., is the limiting reagent), then the reaction will stop.
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The limiting reagent in Reaction (1) is the one that is completely consumed first. This depends on the initial concentrations of the reagents and the stoichiometry of the reaction. Without this information, it's not possible to definitively say which reagent is the limiting one.
Similar Questions
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