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) +…”
Answer
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Answer:
Explanation:
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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:

Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
H^{o}_{rxn.}
= [ ( 1.0 mol ) x (
H_{f}^{o} [ CH3CHO(g)) ] ) + (1.0 mol ) x (
H_{f}^{o} [O2(g) ] ) ] – [ (
H_{f}^{o}[ C2H4 (g) ] +
H_{f}^{o}[ O3 (g) ) ]
H^{o}_{rxn.} = [? (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
H^{o}_{rxn.} = – 366.0 kJ /
mol
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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:

Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
H^{o}_{rxn.}
= [ ( 1.0 mol ) x (
H_{f}^{o} [ NO2(g)) ] ) + (1.0 mol ) x (
H_{f}^{o} [O2(g) ] ) ] – [ (
H_{f}^{o}[ O3 (g) ] +
H_{f}^{o}[ NO(g) ) ]
HTML3_ H^{o}_{rxn.} = [ (1.0 mole) x (+ 33.2kJ/mole) x(0.0 kJ/mole) ]– [ $1.0 mole) x (+143.0kJ/mole) + (1.0mole) ] = – 200.09 kJ /
mol
H^{o}_{rxn.} = – 200.09 kJ /
mol
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Part
– (c):
 Given:

balanced
chemical equation: SO3 (g) + H2O (l)H2SO4 (aq) ————Equation –
3

Step – 1:
We now know the standard enthalpy of formation of the given: reactants, products:

Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
H^{o}_{rxn.}
= [ ( 1.0 mol ) x (
H_{f}^{o} [H2SO4 (aq) ] ) ] – [ (
H_{f}^{o}[ SO3 (g) ] +
H_{f}^{o}[ H2O (l) ) ]
H^{o}_{rxn.} = [? ( 1.0 Mol) x [814.0 KJ/mol () ]) ]– [? (1.0 Mol) x (+ (1.0 Mol) x + (285.8 (kJ/mol) ]
= – 132.5
kJ / mol
H^{o}_{rxn.} = – 132.5 kJ /
mol
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Part
– (d):
 Given:

Step – 1:
We now know the standard enthalpy of formation of the given: reactants, products:

Step – 2:
Therefore, according to Equation – 1: the value of the standard
change of enthalpy: of Equation – 1, will be the following;
H^{o}_{rxn.}
= [ ( 2.0 mol ) x (
H_{f}^{o} [NO2 (g) ] ) ] – [ ( 2.0 mol ) x (
H_{f}^{o}[ NO(g) ] + ( 1.0 mol ) x (
H_{f}^{o}[ O2 (g)) ]
H^{o}_{rxn.} = [ (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
H^{o}_{rxn.} = – 114.18 kJ /
mol
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Conclusion
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