For a particular redox reaction, NO-2 is oxidized to NO-3 and Ag+ is reduced to Ag . Complete and balance the equation for this reaction in basic solution. The phases are optional. balanced reaction: NO-2 + Ag^{+} -> NO-3+ Ag

The following are the steps  to complete and balnce the equation for the given reaction

Explanation:

We are given, NO2– is oxidized to NO3– and Ag is reduced to Ag

NO2– + Ag+ > NO3– + Ag(s)

Step 1) Assign the oxidation state to each element reaction

NO2– + Ag+ > NO3– + Ag(s)

N= +3                           N = +5                        

O = -2                            O = -2

Ag = +1                         Ag = 0

NO2– > NO3– ………oxidation half reaction

Ag+ > Ag(s) ……….reduction half reaction

Step 2) Balance the element other than O and H

     NO2– > NO3–

     Ag+ > Ag(s)

Step 3) Balance the O by adding 1 H2O for 1 O

     NO2– + H2O > NO3–

     Ag+ > Ag(s)

Step 4) Balance the H by adding H+

    NO2– + H2O > NO3– + 2H+

     Ag+ > Ag(s)

Step 5) Balance the charge by adding electron

    NO2– + H2O > NO3– + 2H+ + 2e-

     Ag+ + 1e> Ag(s)

Step 6) Balance the electron in both half reaction

    NO2– + H2O > NO3– + 2H+ + 2e-

     2 Ag+ + 2e> 2 Ag(s)

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

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