Question

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).

Answer #1

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

Get

**2 SO2(g) + O2(g) → 2 SO3(g)**

NOTE: do not add equation 3, we can't cnacel H2SO4

only use 1 and 2

2 S(s) + 3 O2(g) → 2 SO3(g) ΔH = −790 kJ

S(s) + O2(g) → SO2(g) ΔH = −297 kJ

invert (2)

2 S(s) + 3 O2(g) → 2 SO3(g) ΔH = −790 kJ

SO2(g) →S(s) + O2(g) ΔH = +297 kJ

Mulitlpy (2) by 2

2 S(s) + 3 O2(g) → 2 SO3(g) ΔH = −790 kJ

2SO2(g) →2S(s) + 2O2(g) ΔH = 2*(297) = 594 kJ

add all equations

2 S(s) + 3 O2(g) + 2SO2(g) → 2 SO3(g) + 2S(s) + 2O2(g) ΔH = −790 + 594 kJ = -196 kJ

cancel common terms

O2(g) + 2SO2(g) → 2 SO3(g) ΔH = -196 kJ

its the same as

**2 SO2(g) + O2(g) → 2 SO3(g)**

**then ΔH = -196 kJ**

Given the following reactions
2S (s) + 3O2 (g) → 2SO3
(g) ΔH = -790 kJ
S (s) + O2 (g) → SO2(g) ΔH = -297
kJ
the enthalpy of the reaction in which sulfur dioxide is oxidized to
sulfur trioxide
2SO2 (g) + O2 (g) →
2SO3 (g)
is ________ kJ.

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)

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)

Use the standard reaction enthalpies given below to determine
ΔH°rxn for the following reaction:
2 S(s) + 3 O2(g) → 2 SO3(g) ΔH°rxn = ?
Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ 2 SO2(g) + O2(g)
→ 2 SO3(g) ΔH°rxn = -197.8 kJ
Please explain in detail.

Given the following thermochemical data:
½H2(g)+AgNO3(aq) → Ag(s)+HNO3(aq) ΔH = -105.0 kJ
2AgNO3(aq)+H2O(l) → 2HNO3(aq)+Ag2O(s) ΔH = 44.8 kJ
H2O(l) → H2(g)+½O2(g) ΔH = 285.8 kJ
Use Hess’s Law to determine ΔH for the reaction:
Ag2O(s) → 2Ag(s)+½O2(g)

Ex: For the reaction: 2 SO2(g) + O2(g) 2 SO3(g) at 25C and 1
atm.,
what are delta H, delta S, and delta G, given:
deltaH delta S
SO2(g) -297 kJ/mole 248 J/moleK
SO3(g) -396 257
O2(g) 0 205
Hf S SO2(g) -297 kJ/mole 248 J/moleK SO3(g) -396 257 O2(g) 0
205

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)

Use Hess's Law to calculate the enthalpy of reaction, ΔH rxn,
for the reaction in bold below given the following chemical steps
and their respective enthalpy changes. Show ALL work!
2 C(s) + H2(g) → C2H2(g) ΔH°rxn = ?
1. C2H2(g) + 5/2 O2(g) → 2CO2 (g) + H2O (l) ΔH°rxn = -1299.6
kJ
2. C(s) + O2(g) → CO2 (g) ΔH°rxn = -393.5 kJ
3. H2(g) + ½ O2(g) → H2O (l) ΔH°rxn = -285.8 kJ

Use the ΔHrxn values of the following reactions:
2 SO2 (g) + O2 (g) → 2 SO3 (g) ΔHrxn = -196 kJ
1/4 S8 (s) + 3 O2 (g) → 2 SO3 (g) ΔHrxn = -790 kJ
to calculate the ΔHrxn value of this reaction:
1/8 S8 (s) + O2 (g) → SO2 (g)

Use the ΔHrxn values of the following reactions:
2 SO2 (g) + O2 (g) → 2 SO3 (g) ΔHrxn = -196 kJ
1/4 S8 (s) + 3 O2 (g) → 2 SO3 (g) ΔHrxn = -790 kJ
to calculate the ΔHrxn value of this reaction: 1/8 S8 (s) + O2
(g) → SO2 (g)

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