Question

The reaction fe (s) cl2 (g)→ fecl2 (s) has a δh=−342kj . how much heat will be required to produce 1 mole of fe by the reverse reaction? responses −342 kj , negative 342, kj −171 kj negative 171, kj 342 kj 342 kj 684 kj

Answer 1

The answer to your question is, D. 684 kj

Step-by-step explanation:

( I really only have one explantion to this.. )

** The reverse reaction of Fe (s) + Cl2 (g) → FeCl2 (s) is FeCl2 (s) → Fe (s) + Cl2 (g). **

The change in enthalpy (ΔH) is the amount of energy released or in other cases absorbed in a series of chemical reactions. In this case, the reaction has a ΔH of -342 kJ, meaning that 342 kJ of energy is now released. To produce 1 mole of Fe by the reverse reaction, 684 kJ of energy has to be absorbed, which is equal to twice the ΔH of -342 kJ.

Thus the correct answer to your problem is, 684 kj