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 ?
What characteristic must a compound have to experience the following intermolecular forces?
London Dispersion Forces
Dipole-dipole forces
Hydrogen bonding
Identify the predominant intermolecular forces in dimethyl ether (CH3OCH3) and ethanol (C2H5OH) and predict which will have the higher boiling point.
Use PV = nRT
n = grams/molar mass.
Calculate P.
For the others, read this.
http://en.wikipedia.org/wiki/Intermolecular_force
PV = nRT does not work there is 2 parts to this question the first part.
If a 100.0 mL spray can contains 1.00 g of benzocaine, calculate the pressure within the can?
And the second part...
explain why it is likely to explode when heated in a fire where the temperature may be as high as 1300oC ?
I beg your pardon. PV = nRT DOES work. That provides at least some information to answer the second part. I didn't answer the second part. Frankly I think the second part is a guess since we don't know how strong the can is; however, I would hazard a guess that at almost 6000 mm Hg pressure it wouldn't survive. And with the word likely in the problem I think the author of the problem expected us to guess. I assumed the student could guess as well.
2.160692 x10 7 atm Is this the correct answer?
Part two is a discussion
Is anyone able to answer this one? I am really struggling..
Identify the predominant intermolecular forces in dimethyl ether (CH3OCH3) and ethanol (C2H5OH) and predict which will have the higher boiling point.
Dimethyl ether = predominate weak dipole-dipole intermolecular force. (positively charged hydrogen atoms and the negatively charged oxygen atoms).
Ethanol = hydrogen bonding (Hydrogen bonding to oxygen)
Hydrogen bonds have higher boiling points
Dimethyl ether = predominate weak dipole-dipole intermolecular force. (positively charged hydrogen atoms and the negatively charged oxygen atoms).
H+ H+
H+- C- O - C - H+
H+ H+
Ethanol = hydrogen bonding (Hydrogen bonding to oxygen)
H+ H+
H+ - C - C - O - H+
H+ H+
Hydrogen bonds have higher boiling points