Question 2 -
Liquid vitamin C, (ascorbic acid) C6H8O6 , readily reacts with atmospheric oxygen, O2, to form liquid dehydroascorbic acid, C6H6O6 and water.
a) Explain why this is a chemical reaction.
b) Write a balanced equation for this reaction.
c) How many mole of oxygen gas is required to react with 1000.0 mg of vitamin C?
d) 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.
e) What is the theoretical yield of dehydroascorbic acid for the reaction of 1000.0 mg of vitamin C with 1.00 g of oxygen?
Question 3 (based on Topic 6 - chapter 7 of text)
a) Solarcaine aerosol spray is used for temporarily relieving pain as it works as a topical anesthetic numbing the skin. Solarcaine is in fact benzocaine, C9H11NO2 with molar mass 165.2 g/mol.
If a 100.0 mL spray can contains 1.00 g of benzocaine, calculate the pressure within the can and explain why it is likely to explode when heated in a fire where the temperature may be as high as 1300oC ?
b) What characteristic must a compound have to experience the following intermolecular forces?
i. London Dispersion Forces
ii. Dipole-dipole forces
iii. Hydrogen bonding
c) Identify the predominant intermolecular forces in dimethyl ether (CH3OCH3) and ethanol (C2H5OH) and predict which will have the higher boiling point.
5 answers
Using the coefficients in the balanced equation, convert mols vit C to mols to mols O2.
that part though
Perhaps the answer can be found in your lecture notes and some internet research rather than cheating by copy-pasting the entire question set onto a forum.
1 answer