For each reaction, calculate how many moles of product form when 1.75 mol of the reactant in color completely reacts. Assume there is more than enough of the other reactant. (a) (b) (c) (d) 2 S(s) + 3 O2(g) 2 SO3(g) 2 Na(s) + O2(g) Na2O2(s) 2 H2(g) + O2(g) 2 H2O(l) H2(g) + Cl2(g) 2 HCl(g)
Intermolecular Forces - Molecules leave surface of liquids and enter gas state; re-enter liquid phase through surface - When vapor pressure = room pressure, the liquid is then boiling - Compounds are held together by different forces - Dipole- no + or -; distributed evenly - Hydrocarbons are always nonpolar - Van der Waal’s forces: attractive forces that hold particles together in the condensed phases that include dipole-dipole interactions and dispersion forces - Dispersion forces are present in all molecules to hold them together - Dipole attraction must include polar molecules - Hydrogen bonding occurs in molecules that contain H bonded to a small electronegative atom - Crystal structure of exte
