Answer: At equilibrium, the partial pressure of 
is 0.0330 atm.
Explanation:
The partial pressure of is equal to the partial pressure of 
. Hence, let us assume that x quantity of 
is decomposed and gives x quantity of and x quantity of .
Therefore, at equilibrium the species along with their partial pressures are as follows.
At equilibrium: 0.123-x x x
Now, expression for 
of this reaction is as follows.
![K_{p} = \frac{[PCl_{3}][Cl_{2}]}{[PCl_{5}]}\\0.0121 = \frac{x \times x}{(0.123 - x)}\\x = 0.0330](https://tex.z-dn.net/?f=K_%7Bp%7D%20%3D%20%5Cfrac%7B%5BPCl_%7B3%7D%5D%5BCl_%7B2%7D%5D%7D%7B%5BPCl_%7B5%7D%5D%7D%5C%5C0.0121%20%3D%20%5Cfrac%7Bx%20%5Ctimes%20x%7D%7B%280.123%20-%20x%29%7D%5C%5Cx%20%3D%200.0330)
Thus, we can conclude that at equilibrium, the partial pressure of is 0.0330 atm.
Fully donating an electron results in an ionic bond, so A is the correct answer.
In comparison, B, a hydrogen bond, is a bond that forms between an H in one compound and an O, N, or F in another. It is among the strongest of intermolecular forces, while ionic/covalent bonds are intramolecular.
C, a covalent bond, is a bond that forms when atoms share electrons instead of donating them.
Answer:
7.81 moles
Explanation:
(4.7×10^24 )×1 moles divided by 6.02×10^23 molecules
