What is the predominant intermolecular force in the liquid state of each of these compounds: methanol (ch3oh), carbon tetrafluoride (cf4), and hydrogen sulfide (h2s)? drag the appropriate items to their respective bins. dipole-dipole forces- hydrogen bonding- dispersion forces-?

The inter-molecular forces are the force of attraction between molecules.

Hydrogen bond : it is an effective force of attraction between a highly electronegative element (F, O or N) and a hydrogen bonded to a highly electronegative element (F, O or N).

Dipole dipole force: it is present in polar molecules.

Dispersion force: these forces are present in all molecules however in non polar molecules this force of attraction is primary force.

Methanol : hydrogen bond

carbon tetrafluoride : dispersion force

Hydrogen sulfide : dipole-dipole forces

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml

a 20-cm-long, cylindrical graphite (pure carbon) rod is inserted into an oxidizing atmosphere at 1145 k and 1.013 x 105 pa pressure. the oxidizing process is limited by the diffu- sion of oxygen counterflow to the carbon monoxide that is formed on the cylindrical surface.