Calculate AH° for each of the following reactions, which occur in the atmosphere. (a) C2H4(g) +…
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Question “Calculate AH° for each of the following reactions, which occur in the atmosphere. (a) C2H4(g) +…”
Calculate AH° for each of the following reactions, which occur in the atmosphere. (a) C2H4(g) + O3(g) → CH3CHO(g) + O2(g) СkJ (b) 03(g) + NO(g) → NO2(g) + O2(g) (c) SO3(g) + H20(1) – H2SO4(aq) Гk) (d) 2 NO(g) + O2(g) → 2 NO2(g) k]
Answer
Following is
theComplete Answer-&- Explanation for the given: Question in strongTag4$
Answer:
part –
(a):Horxn. = – 366.0 kJ /
mol
part – (b): Horxn. = – 200.09 kJ /
mol
part – (c): Horxn. = – 132.5 kJ /
mol
part – (d):Horxn. = – 114.18 kJ /
mol
Explanation:
The complete : Explanation: For the above: $strongTag16
————————————————————————————————–
Part
– (a):
Given:
balanced chemical
equation: C2H4 (g) + O3 (g)
CH3CHO (g) + O2 (g) ————-Equation – 1
Step – 1:
We now know the standard enthalpy of formation of the given: reactants, products:
Hfo
[ C2H4 (g) ] = + 52.3 kJ /
mol
Hfo
[ O3 (g) ] = + 143.0 kJ / mol
Hfo
[ CH3CHO(g) ] = -170.7 kJ /
mol
Hfo
[O2(g) ] = 0.0 kJ / mol
Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
Horxn.
= [ ( 1.0 mol ) x (
Hfo [ CH3CHO(g)) ] ) + (1.0 mol ) x (
Hfo [O2(g) ] ) ] – [ (
Hfo[ C2H4 (g) ] +
Hfo[ O3 (g) ) ]
Horxn. = [? (1.0 mole) x [-170.7 kJ/mole]??) x (0.0 kJ/mole) ][ 1.0 mole) x (52.3kJ/mole) + (1.0 Mole) x (] = – 366.0 kJ /
mol
Horxn. = – 366.0 kJ /
mol
—————————————————————————————————
Part
– (b):
Given:
balanced
chemical equation: O3 (g) + NO (g)
NO2 (g) + O2 (g) ————-Equation – 2
Step – 1:
We now know the standard enthalpy of formation of the given: reactants, products:
Hfo
[ NO2 (g) ] = + 33.2 kJ / mol
Hfo
[ O3 (g) ] = + 143.0 kJ / mol
Hfo
[NO(g) ] = +90.29 kJ / mol
Hfo
[O2(g) ] = 0.0 kJ / mol
Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
We now know the standard enthalpy of formation of the given: reactants, products:
Hfo
[H2SO4 (aq) ] = -814.0 kJ /
mol
Hfo
[ SO3 (g) ] = −395.7kJ /
mol
Hfo
[H2O (l) ] = −285.8kJ /
mol
Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
Horxn.
= [ ( 1.0 mol ) x (
Hfo [H2SO4 (aq) ] ) ] – [ (
Hfo[ SO3 (g) ] +
Hfo[ H2O (l) ) ]
Horxn. = [? ( 1.0 Mol) x [-814.0 KJ/mol () ]) ]– [? (1.0 Mol) x (+ (1.0 Mol) x + (-285.8 (kJ/mol) ]
= – 132.5
kJ / mol
Horxn. = – 132.5 kJ /
mol
——————————————————————————————————
Part
– (d):
Given:
balanced
chemical equation: 2 NO (g) + O2 (g) 2 NO2 (g) ————-Equation –
3
Step – 1:
We now know the standard enthalpy of formation of the given: reactants, products:
Hfo
[ NO2 (g) ] = + 33.2 kJ / mol
Hfo
[NO(g) ] = +90.29 kJ / mol
Hfo
[O2(g) ] = 0.0 kJ / mol
Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
Horxn.
= [ ( 2.0 mol ) x (
Hfo [NO2 (g) ] ) ] – [ ( 2.0 mol ) x (
Hfo[ NO(g) ] + ( 1.0 mol ) x (
Hfo[ O2 (g)) ]
Horxn. = [ (2.0 Mol) x (+33.2 kJ/mol) ]) ]– [(2.0 Mol) x (+90.29 KJ/mol) + (1.0 Mol) x (0.0kJ/mol ]
= – 114.18
kJ / mol
Horxn. = – 114.18 kJ /
mol
——————————————————————————————————-
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Conclusion
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