Following is the - complete Answer -&- Explanation: for the given: Question: in...typed format...
Answer:
Explanation:
Following is the complete : Explanation: for the above: Answer...
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Part - (a):
Now, we know the following standard enthalpy of formation: of the given: reactants and products:
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 mol ) x (-170.7 kJ / mol ) ] ) + (1.0 mol ) x (0.0 kJ/mol ) ] - [ ( 1.0 mol) x (52.3 kJ / mol ] + (1.0 mol ) x ( 143.0 kJ / mol ) ] = - 366.0 kJ / mol
Horxn. = - 366.0 kJ / mol
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Part - (b):
Now, we know the following standard enthalpy of formation: of the given: reactants and products:
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 [ NO2(g)) ] ) + (1.0 mol ) x (Hfo [O2(g) ] ) ] - [ ( Hfo[ O3 (g) ] + Hfo[ NO(g) ) ]
Horxn. = [ ( 1.0 mol ) x (+ 33.2 kJ / mol ) ] ) + (1.0 mol ) x (0.0 kJ/mol ) ] - [ ( 1.0 mol) x (+ 143.0 kJ / mol ] + (1.0 mol ) x ( +90.29 kJ / mol ) ] = - 200.09 kJ / mol
Horxn. = - 200.09 kJ / mol
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Part - (c):
Now, we know the following standard enthalpy of formation: of the given: reactants and products:
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 (−395.7 kJ / mol ) + (1.0 mol ) x (−285.8 kJ / mol ) ]
= - 132.5 kJ / mol
Horxn. = - 132.5 kJ / mol
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Part - (d):
Now, we know the following standard enthalpy of formation: of the given: reactants and products:
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 (0.0 kJ/mol) ]
= - 114.18 kJ / mol
Horxn. = - 114.18 kJ / mol
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Calculate AH° for each of the following reactions, which occur in the atmosphere. (a) C2H4(g) +...
Calculate ΔH° for each of the following reactions, which occur in the atmosphere.(a) C2H4(g) + O3(g) → CH3CHO(g) + O2(g)(b) O3(g) + NO(g) → NO2(g) +O2(g)(c) SO3(g) + H2O(l) → H2SO4(aq)(d) 2 NO(g) + O2(g) → 2 NO2(g)
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Watch video tutorial on Blackboard Calculate AH for each of the following reactions (use the data in Appendix II): (a) 2 C4H10 (g) + 13 O2(g) → 8 CO2(g) + 10 H20(g) (b) 4 NH3(g) + 5 O2() 4 NO(g) + 6 H20()
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