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
the Complete Answer-&- Explanation for the given: Question in strongTag4$

Answer:

1. part –
   (a):

   

   H^o_rxn. = – 366.0 kJ /
   mol

2. part – (b):
     

   

   H^o_rxn. =  – 200.09 kJ /
   mol

3. part – (c):
     

   

   H^o_rxn. =  – 132.5 kJ /
   mol

4. part – (d):

   

   H^o_rxn. =  – 114.18 kJ /
   mol

Explanation:

The complete : Explanation: For the above: $strongTag16

————————————————————————————————–

Part
– (a):

• Given:

1. 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:

1. 

   H_f^o
   [ C₂H₄ (g) ] = + 52.3 kJ /
   mol

2. 

   H_f^o
   [ O₃ (g) ] = + 143.0 kJ / mol

3. 

   H_f^o
   [ CH₃CHO(g) ] = -170.7  kJ /
   mol

4. 

   H_f^o
   [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;

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

—————————————————————————————————

Part
– (b):

• Given:

1. 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:

1. 

   H_f^o
   [ NO₂ (g) ] = + 33.2 kJ / mol

2. 

   H_f^o
   [ O₃ (g) ] = + 143.0 kJ / mol

3. 

   H_f^o
   [NO(g) ] = +90.29 kJ / mol

4. 

   H_f^o
   [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;

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

—————————————————————————————————-

Part
– (c):

• Given:

1. 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:

1. 

   H_f^o
   [H₂SO₄ (aq) ] = -814.0 kJ /
   mol

2. 

   H_f^o
   [ SO₃ (g) ] = −395.7 kJ /
   mol

3. 

   H_f^o
   [H₂O (l) ] = −285.8 kJ /
   mol

• 
  ​​​​​​​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

——————————————————————————————————

Part
– (d):

• Given:

1. 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:

1. 

   H_f^o
   [ NO₂ (g) ] = + 33.2 kJ / mol

2. 

   H_f^o
   [NO(g) ] = +90.29 kJ / mol

3. 

   H_f^o
   [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;

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

——————————————————————————————————-

Conclusion

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