The third shell has 3 subshells: the subshell, which has 1 orbital with 2 electrons, the subshell, which has 3 orbitals with 6 electrons, and the subshell, which has 5 orbitals with 10 electrons, for a total of 9 orbitals and 18 electrons.
Answer:
I think it would be the last answer
Explanation:
<u>Answer: </u>The equation which is wrong is 
<u>Explanation:</u>
For the given reaction:
The expression for 
is given by:
![K_c=\frac{1}{[O_2]^3}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B1%7D%7B%5BO_2%5D%5E3%7D)
![K_p=\frac{1}{[O_2]^3}](https://tex.z-dn.net/?f=K_p%3D%5Cfrac%7B1%7D%7B%5BO_2%5D%5E3%7D)
The concentration of solids are taken to be 1, only concentration of gases and liquid states are taken. The pressure of only gases are taken.
Relationship between 
is given by the expression:
where,
= number of moles of gaseous products - number of moles of gaseous reactants
R = gas constant
T= temperature
For the above reaction,
= number of moles of gaseous products - number of moles of gaseous reactants = 0 - 3 = -3
Hence, the expression for 
is:
Therefore, the equation which is wrong is
Part (a) :
H₂(g) + I₂(s) → 2 HI(g)
From given table:
G HI = + 1.3 kJ/mol
G H₂ = 0
G I₂ = 0
ΔG = G(products) - G(reactants) = 2 (1.3) = 2.6 kJ/mol
Part (b):
MnO₂(s) + 2 CO(g) → Mn(s) + 2 CO₂(g)
G MnO₂ = - 465.2
G CO = -137.16
G CO₂ = - 394.39
G Mn = 0
ΔG = G(products) - G(reactants) = (1(0) + 2*-394.39) - (-465.2 + 2*-137.16) = - 49.3 kJ/mol
Part (c):
NH₄Cl(s) → NH₃(g) + HCl(g)
ΔG = ΔH - T ΔS
ΔG = (H(products) - H(reactants)) - 298 * (S(products) - S(reactants))
= (-92.31 - 45.94) - (-314.4) - (298 k) * (192.3 + 186.8 - 94.6) J/K
= 176.15 kJ - 84.78 kJ = 91.38 kJ
