Solarcaine aerosol spray is used for temporarily relieving pain as it works as a

ID: 870700 • Letter: S

Question

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.

Explanation / Answer

C9H11NO2 with molar mass 165.2 g/mol

The ideal gas law

PV=nRT

P = pressure

V = volume of container

n = amount of substance of gas (the mole volume...you'll probably Avogadro's constant)

R= ideal gas constant )8.314?472 J mol-1 K-1 )

T = Temperature in Kelvin (the absolute temperature)

n= 1X1/165.2

= 0.0006

R= 8.314?472 J mol-1 K-1

T= 1300oC; 1573.15 Kelvin

V=100

= 0.0006 X 8.314X 1573.15/ 100

=7.84 pascal

Benzocaine is the ethyl ester of p-aminobenzoic acid (PABA). As with most organic solids, fire is possible at elevated temperatures or by contact with an ignition source. Contact with strong oxidizers may cause fire.

Explosion:
Benzocaine is a potential dust explosion hazard. . Data is not available on the minimum explosive concentration.

The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction.

Dipole-dipole forces are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

A hydrogen bond is the electrostatic attraction between polar molecules that occurs when ahydrogen (H) atom bound to a highly electronegative atom such as nitrogen (N), oxygen (O) or fluorine (F) experiences attraction to some other nearby highly electronegative atom.

Ethanol and dimethyl ether have the exact same formula but ethanol's boiling point is 78C and dimethyl ether is -25C. This is because in ethanol, the hydrogen and the oxygen are bonded, which results in a large electronegativity difference. This allows hydrogen bonding to occur. However, in dimethyl ether, the oxygen is bonded to a carbon and the electronegativity difference is small. Due to this, ethers form only dipole dipole attractions rather than hydrogen bonds. This is why ethanols have higher boiling point because they need more energy input in order to break those hydrogen bonds.