Question

Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) given the following reactions and enthalpies of formation: 12N2(g)+O2(g)→NO2(g),   ΔH∘A=33.2...

Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g)

given the following reactions and enthalpies of formation:

12N2(g)+O2(g)→NO2(g),   ΔH∘A=33.2 kJ

12N2(g)+12O2(g)→NO(g),  ΔH∘B=90.2 kJ

Homework Answers

Answer #1

2NO(g)+O2(g) → 2NO2(g) ; H = ?                   --------------------- (1)

Given reactions are

1/2N2(g)+O2(g) → NO2(g),   ΔHA =33.2 kJ            --------------------------(2)

1/2N2(g)+1/2O2(g) → NO(g),  ΔHB =90.2 kJ          -------------------------(3)

Eqn(1) can be obtained from Eqn(2) & Eqn(3) as follows :

Eqn(1) = [2x Eqn(1)] + [2xreverse of Eqn(2) ]

So H = (2x ΔHA ] + [2x(-ΔHB )]

             = (2x33.2 kJ ) + [2x(-90.2 kJ)]

            = -114.0 kJ

Therefore the enthalpy of the reaction is -114.0 kJ

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
The standard heat of formation, ΔH∘f, is defined as the enthalpy change for the formation 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...
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...
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...
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...
Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) Then the standard heat of reaction for the overall reaction...
Consider, for example, the reaction 2NO(g)+O2(g)⇌2NO2(g) Then the standard heat of reaction for the overall reaction is ΔH∘rxn=ΔH∘f(products)−−ΔH∘f(reactants) ΔH∘rxn=2(33.2)-[2(90.2)+0]= -114kJ 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. Na(s)+12Cl2(l)→NaCl(s) 2Na(s)+Cl2(g)→2NaCl(s) Na(s)+12Cl2(g)→NaCl(s) H2(g)+12O2(g)→H2O(g) 2H2(g)+O2(g)→2H2O(g) H2O2(g)→12O2(g)+H2O(g) Part B The combustion of heptane, C7H16, occurs via the reaction C7H16(g)+11O2(g)→7CO2(g)+8H2O(g) with heat of formation values given by the following...
Hess's law states that "the heat released or absorbed in a chemical process is the same...
Hess's law states that "the heat released or absorbed in a chemical process is the same whether the process takes place in one or in several steps." It is important to recall the following rules: When two reactions are added, their enthalpy values are added. When a reaction is reversed, the sign of its enthalpy value changes. When the coefficients of a reaction are multiplied by a factor, the enthalpy value is multiplied by that same factor. Part A Calculate...
Given the following reactions and their enthalpies: ΔH(kJ/mol)−−−−−−−−−−− H2(g)⟶2H(g) +436 O2(g)⟶2O(g) +495 H2+12O2(g)⟶H2O(g) −242 Part A...
Given the following reactions and their enthalpies: ΔH(kJ/mol)−−−−−−−−−−− H2(g)⟶2H(g) +436 O2(g)⟶2O(g) +495 H2+12O2(g)⟶H2O(g) −242 Part A Devise a way to calculate ΔH for the reaction H2O(g)⟶2H(g)+O(g)
Applying Hess’s Law, from the enthalpies of reactions, N2(g) + 3H2(g) → 2 NH3(g) ΔH =...
Applying Hess’s Law, from the enthalpies of reactions, N2(g) + 3H2(g) → 2 NH3(g) ΔH = − 91.8 kJ O2(g) + 2H2(g) → 2H2O (g) ΔH = − 483.7 kJ N2(g) + O2(g) → 2NO(g) ΔH = 180.6 kJ Calculate the enthalpy change (ΔHrxn) for the reaction: 4NH3(g) + 5O2(g) → 4 NO (g) + 6H2O(g)
Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: SO2(g)+12O2(g)→SO3(g) ΔH∘rxn =
Use standard enthalpies of formation to calculate ΔH∘rxn for the following reaction: SO2(g)+12O2(g)→SO3(g) ΔH∘rxn =
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The...
1.) Using enthalpies of formation, calculate the standard change in enthalpy for the thermite reaction. The enthalpy of formation of Fe3O4 is −1117 kJ/mol. 8 Al(s) + 3 Fe3O4(s) → 4 Al2O3(s) + 9 Fe(s) 2. a) Nitroglycerin is a powerful explosive, giving four different gases when detonated. 2 C3H5(NO3)3(l) → 3 N2(g) + 1/2 O2 (g) + 6 CO2(g) + 5 H2O(g) Given that the enthalpy of formation of nitroglycerin, ΔHf°, is −364 kJ/mol, calculate the energy (heat at...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT