Consider the equations below. CH4 (g)->C(s)+2H2(g) H1 = 74.6 kJ

C(s) + 2CI2(g)->CCI4(g) H2 = -95.7 kJ

2H2(g) + 2CI2(g)-> 4HCI(g) H3 = -184.6 kJ

CH4(g) + 4CI2(g) -> CCI4(g) + 4HCI(g) H4 = -205.7 kJ

Complete the following based on the diagram.

Arrow A: 74.6 kJ
-95.7 kJ
-184.6 kJ

Arrow B: endothermic
exothermic

Arrow C: - bas a magnitude that is greater than that of B
- has a magnitude that is less than that of B
- has negative enthalpy

Arrow D: - represents an intermediate reaction
- has a magnitude that is always higher than any intermediate reaction
- represents the overall enthalpy of reaction