Please provide the full matlab code

Note that this is a group project. Please submit 1. Written report and corresponding m files. 2. Peer evaluation forms Background: Data for the partial pressure of carbon dioxide (CO2) collected at Mauna Loa, Hawaii from 1958 through 2003 indicates that levels have increased over 19% during the period from 315 to 376ppm. The trend in the data can be nicely fit with a quadratic polynomial: pCO2=0.011825(t1980.5)2+1.356975(t1980.5)+339 where pCO2 is the partial pressure of CO2 in the atmosphere [ppm]. The increase of carbon dioxide can also influence atmospheric chemistry. Outside of urban and industrial areas, it is well documented that carbon dioxide is the primary determinant of the pH of the rain. pH is the measure of the activity of hydrogen ions and, therefore, its acidity. For dilute aqueous solutions, it can be computed as pH=log10[H+] where [H+]is the molar concentration of hydrogen ions. The following five nonlinear system of equations govern the chemistry of rainwater, K1K2KwcT0=106KHPCO2[H+][HCO3]=[HCO3][H+][CO32]=[H+][OH]=106KHPCO2+[HCO3]+[CO32]=[HCO3]+2[CO32]+[OH][H+] where KH= Henry's constant, and K1,K2 and Kw are equilibrium coefficients. The five unknowns are cT= total inorganic carbon, [HCO3]= bicarbonate, [CO3]= carbonate, [H+]=hydrogen ion, and [OH]=hydroxyl ion. In this case study, we will examine how the carbon dioxide trend affects the pH of rainwater by using the data for the partial pressure of carbon dioxide collected (Eq.1) The pH of rainwater can be computed based on Eq. 3 given that KH=101.46,K1=106.3,K2= 1010.3, and Kw=1014. Please also consider the following: - The pH of rain in pristine areas always falls between 2 and 12 . - Typical measurement devices can only measure pH to two places of decimal precision