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?
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.
@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
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
This is a chemical reaction because the reactants (liquid vitamin C and atmospheric oxygen) react together to form new substances (liquid dehydroascorbic acid and water). In a chemical reaction, bonds are broken and formed between atoms, resulting in the rearrangement of atoms to create new molecules.
The balanced equation for this reaction is:
C6H8O6 + O2 -> C6H6O6 + H2O
To determine how many moles of oxygen gas is required to react with 1000.0 mg of vitamin C, we need to convert the mass of vitamin C to moles. The molar mass of vitamin C (ascorbic acid) is 176.12 g/mol (6 * 12.01 g/mol for carbon + 8 * 1.01 g/mol for hydrogen + 6 * 16.00 g/mol for oxygen). Using this molar mass, we can calculate:
1000.0 mg (1 g / 1000 mg) (1 mol / 176.12 g) = 0.00568 mol
According to the balanced equation, 1 mole of oxygen is required to react with 1 mole of vitamin C. Therefore, 0.00568 mol of oxygen gas is required to react with 1000.0 mg of vitamin C.
To determine if 1.00 g of oxygen is enough to completely react with the 1000.0 mg of vitamin C, we need to compare the molar amounts of oxygen and vitamin C. The molar mass of oxygen gas (O2) is 32.00 g/mol. Converting the mass of oxygen to moles:
1.00 g (1 mol / 32.00 g) = 0.03125 mol
Since we have more moles of oxygen (0.03125 mol) than the required amount (0.00568 mol), oxygen is in excess and would not be completely consumed. Therefore, 1.00 g of oxygen is more than enough to react with 1000.0 mg of vitamin C.
The theoretical yield of dehydroascorbic acid can be calculated based on the limiting reagent. The limiting reagent is the reactant that is completely consumed first and determines the maximum amount of product that can be formed. In this case, the limiting reagent can be identified by comparing the moles of reactants.
From previous calculations, we found that we have 0.00568 mol of vitamin C and 0.03125 mol of oxygen. According to the balanced equation, the mole ratio between vitamin C and dehydroascorbic acid is 1:1. Therefore, the maximum moles of dehydroascorbic acid that can be formed is also 0.00568 mol.
To calculate the theoretical yield of dehydroascorbic acid in grams, we need to use its molar mass, which is 174.12 g/mol. Multiplying the molar mass by the number of moles:
0.00568 mol * 174.12 g/mol = 0.9883 g
Therefore, the theoretical yield of dehydroascorbic acid for the reaction of 1000.0 mg of vitamin C with 1.00 g of oxygen is 0.9883 grams.