Energetics chem question
Two reactions of iron with oxygen are shown.
Fe(s) + O2(g) → FeO(s) ΔH = – 272 kJ mol–1
2 Fe(s) + O2(g) → Fe2O3(s) ΔH = – 822 kJ mol–1
What is the enthalpy change, in kJ mol–1
, for this reaction?
2 FeO(s) + O2(g) → Fe2O3(s)
A +550
B –278
C –1094
D –1372
Answer= B, but how do you go about calculating the answer when multiple equations are given?
Fe(s) + O2(g) → FeO(s) ΔH = – 272 kJ mol–1
2 Fe(s) + O2(g) → Fe2O3(s) ΔH = – 822 kJ mol–1
What is the enthalpy change, in kJ mol–1
, for this reaction?
2 FeO(s) + O2(g) → Fe2O3(s)
A +550
B –278
C –1094
D –1372
Answer= B, but how do you go about calculating the answer when multiple equations are given?
you are told the enthalpy of formation of FeO from the first equation so 2FeO would b 2 x -272. oxygen is an element so has no value. you are also told the enthalpy of formation of Fe2O3 which is -822. then just draw a normal hess cycle
Original post by B7861
you are told the enthalpy of formation of FeO from the first equation so 2FeO would b 2 x -272. oxygen is an element so has no value. you are also told the enthalpy of formation of Fe2O3 which is -822. then just draw a normal hess cycle
Thank you
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