Covalent compounds are known to have low melting point because they have weak forces of attraction between the binding molecules, so low amount of energy is needed to break the binding force.
The untrue statement is that they high melting points.
The covalent compounds are the compounds exhibiting strong intra-molecular bonds. This is due to the tightness of the atoms within the covalent molecules. The force of attraction between the individual molecules in a covalent compound seems to be weak. The covalent compounds exhibit weak intermolecular forces that hold the atoms together due to this they have a low melting point.
Use the ideal gas law: <em>PV=nRT </em>p = pressure v = volume n = number of moles of sample R = ideal gas constant = ~0.08206 (l*atm)/(K*mole) T = Temp in Kelvin
Now we substitute while simultaneously solving for P(pressure) P = (nRT)/V P = (2.50 * 0.08206 * (27+273.15)) / 50 P = Now it's your turn.
