Question

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. Check all that apply. 1)Li(s)+12F2(l)→LiF(s)

.2) SO3(g)→12O2(g)+SO2(g).

3) SO(g)+12O2(g)→SO2(g)

. 4) 2Li(s)+F2(g)→2LiF(s).

5)S(s)+O2(g)→SO2(g)

.6) Li(s)+12F2(g)→LiF(s)

Answer #1

answer :

S(s) + O2(g) ------------> SO2(g)

Li(s) + 1/2 F2(g)----------> LiF(s)

Explanation :

The standard enthalpy of formation is defined as the change in enthalpy when one mole of a substance in the standard state (1 atm of pressure and 298.15 K) is formed from its pure elements under the same conditions.

remaing all are not :

ΔH∘rxn = ΔH∘f products - ΔH∘f reactants.

for above two reactions :

ΔH∘rxn = ΔH∘f products. because enthalpyof elemental state of S and F2 and Li are zero.

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.
2Li(s)+F2(g)→2LiF(s)
S(s)+O2(g)→SO2(g)
SO3(g)→12O2(g)+SO2(g)
Li(s)+12F2(l)→LiF(s)
SO(g)+12O2(g)→SO2(g)
Li(s)+12F2(g)→LiF(s)

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...

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.
CO(g)+12O2(g)→CO2(g)
BaCO3(s)→BaO(s)+CO2(g)
Li(s)+12F2(l)→LiF(s)
Li(s)+12F2(g)→LiF(s)
2Li(s)+F2(g)→2LiF(s)
C(s,graphite)+O2(g)→CO2(g)

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.
Check all that apply.
Na(s)+12F2(g)→NaF(s)
SO(g)+12O2(g)→SO2(g)
Na(s)+12F2(l)→NaF(s)
2Na(s)+F2(g)→2NaF(s)
SO3(g)→12O2(g)+SO2(g)
S(s)+O2(g)→SO2(g)

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.
H2(g)+12O2(g)→H2O(g)
Na(s)+12Cl2(g)→NaCl(s)
2Na(s)+Cl2(g)→2NaCl(s)
H2O2(g)→12O2(g)+H2O(g)
Na(s)+12Cl2(l)→NaCl(s)
2H2(g)+O2(g)→2H2O(g)

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...

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 standard heat...

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.

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