Energy E = hc / l
where h = Planck's constant, c = speed of light and l = wavelength.
E = 1.986 * 10^-25 / 3.8 * 10^-7 = 5.223*10^-19
Your answer would be "Chemical Change"
Answer: 
Explanation:
The balanced chemical reaction is,

The expression for Gibbs free energy change is,
![\Delta G_{rxn}=\sum [n\times \Delta G_(product)]-\sum [n\times \Delta G_(reactant)]](https://tex.z-dn.net/?f=%5CDelta%20G_%7Brxn%7D%3D%5Csum%20%5Bn%5Ctimes%20%5CDelta%20G_%28product%29%5D-%5Csum%20%5Bn%5Ctimes%20%5CDelta%20G_%28reactant%29%5D)
![\Delta G_{rxn}=[(n_{CO_2}\times \Delta G_{CO_2})+(n_{CaO}\times \Delta G_{CaO})]-[(n_{CaCO_3}\times \Delta G_{CaCO_3})]](https://tex.z-dn.net/?f=%5CDelta%20G_%7Brxn%7D%3D%5B%28n_%7BCO_2%7D%5Ctimes%20%5CDelta%20G_%7BCO_2%7D%29%2B%28n_%7BCaO%7D%5Ctimes%20%5CDelta%20G_%7BCaO%7D%29%5D-%5B%28n_%7BCaCO_3%7D%5Ctimes%20%5CDelta%20G_%7BCaCO_3%7D%29%5D)
where,
n = number of moles
Now put all the given values in this expression, we get
![\Delta G_{rxn}=[(1\times -394.4)+(1\times -604.17)]-[(1\times -1128.76)]](https://tex.z-dn.net/?f=%5CDelta%20G_%7Brxn%7D%3D%5B%281%5Ctimes%20-394.4%29%2B%281%5Ctimes%20-604.17%29%5D-%5B%281%5Ctimes%20-1128.76%29%5D)

Therefore, the gibbs free energy for this reaction is, +130.19 kJ
5g
Anything between 4 and 6 is ok.