Dichloromethane is produced from two successive chlorination reactions: the chlorination of methane to methyl chloride followed by the chlorination of methyl chloride to dichloromethane. CH, (g) + Cl (g) CH, CI(g) + HCl(g) CH, Cl(g) + Cl2(g) CH,C1(1) + HCl(g) A2 = -134.69 kJ/mol Using the standard heats of formation in the back of your text and the heat of reaction listed, what is the standard heat of formation of CH, CI, 1)? ACH_C1,0) = kJ/mol What is the standard heat of reaction for the combined (overall) reaction? CH,(g) + 2Cl2(g) CH,C1,(1) + 2 HCl(g) A, = kJ/mol If methane and chlorine react to produce 195.0 mol/h of CH,C1, (1), and the reactants and products are at 25 C and 1 atm, how much heat, 0, is evolved or absorbed in the process? Include the appropriate sign. o kJ/h Is this heat evolved or absorbed in the process? absorbed evolved