Use the data below to answer the questions. Substance Delta HF kJ/mol) C(g) 718.4 CF_4(g) -679.9 CH_4(g) -74.8 H(g) 217.94 HF(g) -268.61 Keep in mind that the enthalpy of formation of an element in its standard state is zero. Suppose that 0.650mol of methane, CH4(g), is reacted with 0.800mol of fluorine, F2(g), forming CF4(g) and HF(g) as sole products. Assuming that the reaction occurs at constant pressure, how much heat is released?