Answer :
Dipole moments occur when there is a separation of charge. Dipole moments occur due to atoms electronegativity, where one atom has the ability to attract electrons towards it giving it a negative charge and the one deficient in electrons acquire a positive charge called as the bond moment.
But if the bond moments are equal and opposite in direction , they cancel each other and thus there is no net dipole moment in the molecule.
For example: In carbon dioxide , both the -C=O bonds are polar but as the molecule is linear and the the magnetic moments are equal and oppposite, they cancel each other and the molecule is non polar.
The kc is a representation of how fast the reaction proceeds to their products when it has achieved equilibrium. The activation energy for the forward and the one for the reverse
reaction are similar because they attained chemical equilibrium. A chemical
equilibrium happens when both of the reactant and products achieve the same
concentration. An example is the process of melting and freezing. Melting and freezing for a given
substance occurs at the same temperature. Because the temperature at which the
solid starts to melt is also the temperature at which the liquid starts to
freeze. They are at chemical equilibrium.
Answer:
the molecules of each substance attract each other through dispersion (London) intermolecular force.whether a substance is solid, liquid or gas depends on the balance between the kinetic energies of the molecules and their intermolecular attractions.
thank you.
Answer:
725000
Explanation:
hope you find this helpfull
Answer:
- 
- 
Explanation:
Hello,
In this case, by considering the dissolution of silver bromide:
![AgBr(s)\rightleftharpoons Ag^+(aq)+Br^-(aq) \ \ \ Ksp=[Ag^+][Br^-]=7.7x10^{-13}](https://tex.z-dn.net/?f=AgBr%28s%29%5Crightleftharpoons%20Ag%5E%2B%28aq%29%2BBr%5E-%28aq%29%20%5C%20%5C%20%5C%20Ksp%3D%5BAg%5E%2B%5D%5BBr%5E-%5D%3D7.7x10%5E%7B-13%7D)
And the formation of the complex:
![Ag^+(aq)+2NH_3(aq)\rightleftharpoons Ag(NH_3)_2^+(aq)\ \ \ Kf=\frac{[Ag(NH_3)_2^+]}{[Ag^+][NH_3]^2}=1.6x10^7](https://tex.z-dn.net/?f=Ag%5E%2B%28aq%29%2B2NH_3%28aq%29%5Crightleftharpoons%20Ag%28NH_3%29_2%5E%2B%28aq%29%5C%20%5C%20%5C%20Kf%3D%5Cfrac%7B%5BAg%28NH_3%29_2%5E%2B%5D%7D%7B%5BAg%5E%2B%5D%5BNH_3%5D%5E2%7D%3D1.6x10%5E7)
We obtain the balanced net ionic equation by adding the aforementioned equations:
Now, the equilibrium constant is obtained by writing the law of mass action for the non-simplified net ionic equation:
![AgBr(s)+Ag^+(aq)+2NH_3(aq)\rightleftharpoons Ag(NH_3)_2^+(aq)+Br^-+Ag^+\\\\K=[Ag^+][Br^-]*\frac{[Ag(NH_3)_2^+]}{[Ag^+][NH_3]^2}](https://tex.z-dn.net/?f=AgBr%28s%29%2BAg%5E%2B%28aq%29%2B2NH_3%28aq%29%5Crightleftharpoons%20Ag%28NH_3%29_2%5E%2B%28aq%29%2BBr%5E-%2BAg%5E%2B%5C%5C%5C%5CK%3D%5BAg%5E%2B%5D%5BBr%5E-%5D%2A%5Cfrac%7B%5BAg%28NH_3%29_2%5E%2B%5D%7D%7B%5BAg%5E%2B%5D%5BNH_3%5D%5E2%7D)
So we notice that the equilibrium constant contains the solubility constant and formation constant for the initial reactions:
Best regards.
