Question

Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: SO2(g)+12O2(g)→SO3(g) ΔH∘rxn =

Answer #1

**Solution :-**

formula to calculate the delta H rxn is as follows

Delta H rxn = sum of delta H product – sum of delta H reactant

= [SO3*1] - [SO2*1]

= [-396*1] -[-296.8*1]

**
= -99.2 kJ**

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.

1.Using the enthalpies of formation given below, calculate
ΔH°rxn in kJ, for the following reaction.
Report your answer to two decimal places in standard
notation.
H2S(g) + 2O2(g) → SO3(g) +
H2O(l)
H2S (g): -20.60 kJ/mol
O2 (g): 0.00 kJ/mol
SO3 (g): -395.77 kJ/mol
H2O (l): -285.83 kJ/mol
2. Calculate the amount of heat absorbed/released (in kJ) when
22.54 grams of SO3 are produced via the above
reaction.
Report your answer to two decimal places, and use appropriate signs
to...

The standard heat of formation, ΔH∘f, is defined as the
enthalpy change for the formation of one mole of substance from its
constituent elements in their standard states. Thus, elements in
their standard states have ΔH∘f=0. Heat of formation
values can be used to calculate the enthalpy change of any
reaction.
Consider, for example, the reaction
2NO(g)+O2(g)⇌2NO2(g)
with heat of formation values given by the following table:
Substance
ΔH∘f
(kJ/mol)
NO(g)
90.2
O2(g)
0
NO2(g)
33.2
Then the standard heat...

The standard heat of formation, ΔH∘f, is defined as the
enthalpy change for the formation of one mole of substance from its
constituent elements in their standard states. Thus, elements in
their standard states have ΔH∘f=0. Heat of formation
values can be used to calculate the enthalpy change of any
reaction.
Consider, for example, the reaction
2NO(g)+O2(g)⇌2NO2(g)
with heat of formation values given by the following table:
Substance
ΔH∘f
(kJ/mol)
NO(g)
90.2
O2(g)
0
NO2(g)
33.2
Then the standard heat...

The standard heat of formation, ΔH∘f, is defined as the
enthalpy change for the formation of one mole of substance from its
constituent elements in their standard states. Thus, elements in
their standard states have ΔH∘f=0. Heat of formation
values can be used to calculate the enthalpy change of any
reaction.
Consider, for example, the reaction
2NO(g)+O2(g)⇌2NO2(g)
with heat of formation values given by the following table:
Substance
ΔH∘f
(kJ/mol)
NO(g)
90.2
O2(g)
0
NO2(g)
33.2
Then the heat of...

Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g)
given the following reactions and enthalpies of formation:
12N2(g)+O2(g)→NO2(g), ΔH∘A=33.2 kJ
12N2(g)+12O2(g)→NO(g), ΔH∘B=90.2 kJ

6-56) Use standard enthalpies of formation to calculate ΔHrxn°
for each reaction.
a) 2 H2S(g) + 3 O2(g) ⇒2 H2O(l) + 2 SO2(g)
b) SO2(g) + 12 O2(g) ⇒ SO3(g)
c) C(s) + H2O(g) ⇒ CO(g) + H2(g)
d) N2O4(g) + 4 H2(g) ⇒ N2(g) + 4 H2O(g)

Calculate the standard enthalpy change (ΔH⁰rxn ) for
the reaction of TiCl4(g) and
H2O(g) to form TiO2(s) and
HCl(g) given the standard enthalpies of formation
(ΔH⁰f ) shown in the table below. (Include the sign of the
value in your answer.)
kJ
Compound
ΔH⁰f
(kJ/mol)
TiCl4(g)
−763.2
H2O(g)
−241.8
TiO2(s)
−944.0
HCl(g)
−92.3

At 1000 K , Kp=1.85 for the reaction
SO2(g)+12O2(g)???SO3(g)
What is the value of Kp for the reaction
SO3(g)???SO2(g)+12O2(g)
What is the value of Kp for the reaction
2SO2(g)+O2(g)???2SO3(g)
What is the value of Kc for the reaction in
part (b)?

Part A
For which of the following reactions is ΔH∘rxn equal to
ΔH∘f of the product(s)?
You do not need to look up any values to answer this
question.
Check all that apply.
Hints
Check all that apply.
S(s)+O2(g)→SO2(g)
Li(s)+12F2(g)→LiF(s)
SO(g)+12O2(g)→SO2(g)
SO3(g)→12O2(g)+SO2(g)
2Li(s)+F2(g)→2LiF(s)
Li(s)+12F2(l)→LiF(s)
Part B
The combustion of propane, C3H8, occurs via the reaction
C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)
with heat of formation values given by the following table:
Substance
ΔH∘f
(kJ/mol)
C3H8 (g)
-104.7
CO2(g)
−393.5
H2O(g)
−241.8
Calculate the enthalpy for...

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