Chemistry

Liquid vitamin C, (ascorbic acid) C6H8O6 , readily reacts with atmospheric oxygen, O2, to form liquid dehydroascorbic acid, C6H6O6 and water.

Explain why this is a chemical reaction.

Write a balanced equation for this reaction.

How many mole of oxygen gas is required to react with 1000.0 mg of vitamin C?

Would 1.00 g of oxygen be enough to completely react with the 1000.0 mg of vitamin C? Explain your answer by determining the limiting reagent.

What is the theoretical yield of dehydroascorbic acid for the reaction of 1000.0 mg of vitamin C with 1.00 g of oxygen?

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  1. 1. The original chemical has been changed to something different.

    2C6H8O6 + O2 ==> 2C6H6O6 + 2H2O

    mols vit C = grams/molar mass = 1g/molar mass = ?
    Using the coefficients in the balanced equation, convert mols vit C to mols to mols O2.

    Convert 1.00 g O2 to mols. mols = 1.00/molar mass O2 = ? This gives you the data needed to determine the limiting reagent.

    Using mols of the limiting reagent, convert to mols dehydroascorbic acid formed and convert that to grams. That is the theoretical yield.

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  2. @DrBob222, i am needing assistance for the same questions... i am having trouble understanding the last 3... can i email you or something that would be helpful

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  3. Can someone tell me how to do "Using the coefficients in the balanced equation, convert mols vit C to mols to mols O2." that bit please

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