Question

You are given the following thermodynamic data. 2 Fe(s) + 3/2 O2(g) → Fe2O3(s) ΔH° = -823 kJ 3 Fe(s) + 2 O2(g) → Fe3O4(s) ΔH° = -1120. kJ Calculate the ΔH° for the following reaction. 3 Fe2O3(s) → 2 Fe3O4(s) + ½ O2(g)

Answer #1

**2Fe + 3/2O2 --> Fe2O3 , dH = -823 KJ
..................(1)**

**3Fe + 2O2 ---> Fe3O4 , dH = -1120 KJ
.........................(2)**

**Now 2 times eq 2 - 3 times eq 3 gives
us
( - 3 times eq 3 means we add reverse of eq 3 multiplied by factor
3)**

**6Fe + 4O2 + 3Fe2O3 ---> 2Fe3O4 + 6Fe +
9/2O2**

**net equation is 3F2O3 ( s) --> 2Fe3O4 (s) + 1/2O2 (
g) , dH = 2( -1120) -3( -823) = 229 KJ**

Given the following data:
2Fe(s) + 3CO2(g) → Fe2O3(s) +
3CO(g)
ΔH° = 23.0 kJ
3FeO(s) + CO2(g) → Fe3O4(s) +
CO(g)
ΔH° = -18.0 kJ
3Fe2O3(s) + CO(g) →
2Fe3O4(s) + CO2(g)
ΔH° = -39.0 kJ
Calculate ΔH° for the reaction:
Fe(s) + CO2(g) → FeO(s) + CO(g)

Calculate the ΔH for the following
reaction:
Fe2O3
+ 3 CO → 2 Fe + 3
CO2
based on the reactions below.
3Fe2O3
+
CO→2Fe3O4
+ CO2
ΔH=−48.5kJ
Fe+CO2
→FeO+CO.
ΔH=−11.0kJ
Fe3O4
+CO→3FeO+CO2
ΔH=+22.0kJ

Given the data 2 S(s) + 3 O2(g) → 2 SO3(g) ΔH = −790 kJ S(s) +
O2(g) → SO2(g) ΔH = −297 kJ SO3(g) + H2O(l) → H2SO4(l) ΔH = −132 kJ
use Hess's law to calculate ΔH for the reaction 2 SO2(g) + O2(g) →
2 SO3(g).

Calculate ΔHrxn for the following reaction:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
Use the following reactions and given ΔH′s.
2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH =
-824.2 kJ
CO(g)+1/2O2(g)→CO2(g), ΔH =
-282.7 kJ

Calculate the standard enthalpy change for the reaction
2 Al(s) +
Fe2O3(s)
2
Fe(s) + Al2O3(s)
Given that
2 Al(s) + 3/2 O2
(g)
Al2O3(s) ΔH rxn =
-1669.8 kJ/mol
2 Fe (s) +
3/2 O2
(g)
Fe2O3(s) ΔH rxn = -822.2
kJ/mol

Calculate the enthalpy of reaction (ΔH rxn ) for the following
reaction:
Fe 2 O 3 (s) + 3 CO(g) → 2 Fe(s) + 3 CO 2 (g)
Given:
4 Fe(s) + 3 O 2 (g) → 2 Fe 2 O 3 (s) ΔH = –1648
kJ
2 CO 2 (g) → 2 CO(g) + O2(g) ΔH = +565.4 kJ

Given the following data:
H2(g) + 1/2O2(g) → H2O(l)
ΔH° = -286.0 kJ
C(s) + O2(g) → CO2(g)
ΔH° = -394.0 kJ
2CO2(g) + H2O(l) →
C2H2(g) + 5/2O2(g)
ΔH° = 1300.0 kJ
Calculate ΔH° for the reaction:
2C(s) + H2(g) → C2H2(g)

Hess's Law Given the following data: 2C(s) + 2H2(g) + O2(g) →
CH3OCHO(l) ΔH°=-366.0 kJ CH3OH(l) + O2(g) → HCOOH(l) + H2O(l)
ΔH°=-473.0 kJ C(s) + 2H2(g) + 1/2O2(g) → CH3OH(l) ΔH°=-238.0 kJ
H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ calculate ΔH° for the
reaction: HCOOH(l) + CH3OH(l) → CH3OCHO(l) + H2O(l)

1)Use standard thermodynamic data (in the Chemistry References)
to calculate G at 298.15 K for the following reaction, assuming
that all gases have a pressure of 19.31 mm Hg. 2N2(g) +
O2(g)2N2O(g)
G = ? kJ/mol
2)Using standard thermodynamic data (linked), calculate the
equilibrium constant at 298.15 K for the following reaction.
C2H4(g) + H2O(g)CH3CH2OH(g)
K = ?
3) Calculate the temperature (in kelvins) at which the sign of
G° changes from positive to negative for the reaction below. This...

25.
Calculate the standard enthalpy change for the following
chemical equation.
4FeO (s) + O2 (g) → 2Fe2O3 (s)
Use the following thermochemical equations to solve for the
change in enthalpy.
Fe (s) + ½ O2 (g) → FeO (s) ΔH = -269 kJ/mol
2Fe (s) + 3/2 O2 (g) → Fe2O3
(s) ΔH
= -825 kJ/mol
-2726 kJ/mol
556 kJ/mol
-556 kJ/mol
574 kJ/mol
-574 kJ/mol

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