Liquid vitamin C, (ascorbic acid) C6H8O6 , readily reacts with atmospheric oxygen, O2, to form liquid dehydroascorbic acid, C6H6O6 and water.
How many mole of oxygen gas is required to react with 1000.0 mg of vitamin C?
Chemistry - DrBob222, Wednesday, April 29, 2015 at 10:09pm
balanced equation -> 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.
could someone please explain to me how to do the last bit "Using the coefficients in the balanced equation.... etc... please ive tried for so long and cant do it
Why didn't you show what you had? But thanks for telling us your next problem.
How many mols vit C do you have. That's 1/molar mass = ? and I'll make up a number say 0.1 but of course you know that isn't right. Then you can convert mols of vit C to mols of anything else in the equation by using the coefficients.
0.1 mol vit C x (1 mol O2/2 mol C6H8O6) = 0.1 mol vit C x (1/2) = ? mols O2. It always works that way. mols of what you want go on top and mols of what you have goes on bottom, thus the factor in this case is 1/2. To convert from vit C to mols H2O the factor is 2/2 and for the dehydroascorbic acid the factor is 2/2
To solve this problem, you need to use the coefficients in the balanced equation to convert moles of vitamin C to moles of oxygen gas.
First, calculate the molar mass of vitamin C (ascorbic acid):
C = 12.01 g/mol
H = 1.01 g/mol
O = 16.00 g/mol
Molar mass of vitamin C (C6H8O6) = 6(12.01) + 8(1.01) + 6(16.00) = 176.12 g/mol
Next, convert the mass of vitamin C given in the problem (1000.0 mg) to grams:
1000.0 mg = 1000.0 mg * (1 g/1000.0 mg) = 1.0 g
Now, calculate the moles of vitamin C:
moles of vitamin C = mass of vitamin C / molar mass of vitamin C = 1.0 g / 176.12 g/mol ≈ 0.00568 mol
Finally, use the coefficients in the balanced equation to convert moles of vitamin C to moles of oxygen gas (O2). The balanced equation indicates that 2 moles of vitamin C react with 1 mole of oxygen gas.
moles of O2 = moles of vitamin C * (1 mole of O2 / 2 moles of vitamin C) = 0.00568 mol * (1 mol/ 2 mol) = 0.00284 mol
Therefore, approximately 0.00284 moles of oxygen gas are required to react with 1000.0 mg of vitamin C.