26.5d2,3,4 Final answ enough Tnx **Question 2**The \([Co(NH_3)_5H_2O]^{3+}\) ion has a maximum in its absorption spectrum at 500 nm. Calculate \(\Delta_o\) in kJ/mol.[Text Box]---**Question 3**The \([Co(NH_3)_5H_2O]^{3+}\) ion has a maximum in its absorption spectrum at 500 nm. What color does it absorb?- Green- Orange- Red---**Question 4**How many unpaired electrons would you expect for the complex ion \([Fe(NH_3)_6]^{2+}\) if ammonia acts as a weak-field ligand?A) 5 B) 2 C) 6 D) 4 E) 0 - a - b - c - d - e ---

The answer is 238.4 kJ/mol. In this question, wavelength is given in nm, first convert it into SI unit i.e. in meter. After that use the formula E=hc/(Lambda) to calculate the energy in joules. This calculated energy is for one molecule. For energy in joules/mole, i.e. for one mole, multiply by Avogadro's number 6.022×1023 (since one mole have 6.022×1023 molecules). And then finally convert the answer in kJ/mol (1kJ = 1J) as shown below:-The answer is orange. The given wavelength (500nm) comes under blue region, hence the complex will absorb blue colour light and will emit the light of its complementary colour i.e. orange (Complementary colour of blue is orange). This is why the complex will show orange color.The answer is 4. Since ammonia is acting here as a weak field ligand i.e. it will not pair up the electrons present in the orbitals of iron. And hence the number of electrons that will remain unpair after the complex formation will be 4 as shown below:-