Ch.5 - Thermochemistry

Problem 84a

Chapter 5, Problem 84a

Use bond enthalpies in Table 5.4 to estimate H for each of the following reactions: (a)

Verified step by step guidance

Identify the bonds broken and formed in the reaction. Breaking bonds requires energy (endothermic), while forming bonds releases energy (exothermic).

Use the bond enthalpy values from Table 5.4 to calculate the total energy required to break all the bonds in the reactants.

Calculate the total energy released by forming all the bonds in the products using the bond enthalpy values.

Subtract the total energy released (from forming bonds) from the total energy required (for breaking bonds) to find the overall change in enthalpy (ΔH) for the reaction.

Remember that a negative ΔH indicates an exothermic reaction, while a positive ΔH indicates an endothermic reaction.

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Bond Enthalpy

Bond enthalpy, or bond dissociation energy, is the amount of energy required to break a bond in a molecule in the gas phase. It is typically expressed in kilojoules per mole (kJ/mol) and varies depending on the type of bond and the surrounding atoms. Understanding bond enthalpy is crucial for estimating the energy changes in chemical reactions, as it allows for the calculation of the total energy required to break bonds in reactants and the energy released when new bonds are formed in products.

Hess's Law

Hess's Law states that the total enthalpy change for a reaction is the same, regardless of the number of steps taken to achieve the reaction. This principle allows chemists to calculate the enthalpy change of a reaction by summing the enthalpy changes of individual steps, which can be particularly useful when direct measurement is difficult. In the context of using bond enthalpies, Hess's Law enables the estimation of the overall reaction enthalpy by considering the bonds broken and formed.

Reaction Enthalpy (ΔH)

The reaction enthalpy, denoted as ΔH, represents the change in enthalpy during a chemical reaction. It can be calculated using the formula ΔH = Σ(bond enthalpies of bonds broken) - Σ(bond enthalpies of bonds formed). A positive ΔH indicates an endothermic reaction (energy absorbed), while a negative ΔH indicates an exothermic reaction (energy released). Understanding how to calculate ΔH using bond enthalpies is essential for predicting the energy dynamics of chemical reactions.

Recommended video:

Guided course

02:34

Enthalpy of Formation

Related Practice

Textbook Question

Methanol (CH₃OH) is used as a fuel in race cars. (d) Calculate the mass of CO₂ produced per kJ of heat emitted.

461

views

Textbook Question

Without doing any calculations, predict the sign of H for each of the following reactions: (a) NaCl1s2¡Na+ 1g2 + Cl-1g2

902

views

Open Question

Without doing any calculations, predict the sign of _x001F_H for each of the following reactions: (a) 2 NO2(g) → N2O4(g) (b) 2 F(g) → F2(g) (c) Mg2+(g) + 2 Cl-(g) → MgCl2(s) (d) HBr(g) → H(g) + Br(g)

Open Question

(a) Use enthalpies of formation given in Appendix C to calculate _x001F_H for the reaction Br2(g) → 2 Br(g), and use this value to estimate the bond enthalpy D(Br–Br). (b) How large is the difference between the value calculated in part (a) and the value given in Table 5.4?

Textbook Question

(a) The nitrogen atoms in an N2 molecule are held together by a triple bond; use enthalpies of formation in Appendix C to estimate the enthalpy of this bond, D(N‚N). (b) Consider the reaction between hydrazine and hydrogen to produce ammonia, N2H41g2 + H21g2¡2 NH31g2. Use enthalpies of formation and bond enthalpies to estimate the enthalpy of the nitrogen– nitrogen bond in N2H4. (c) Based on your answers to parts (a) and (b), would you predict that the nitrogen–nitrogen bond in hydrazine is weaker than, similar to, or stronger than the bond in N2 ?

1628

views

Textbook Question

Consider the reaction 2 H₂(g) + O₂(g) → 2 H₂O(l). (a) Use the bond enthalpies in Table 5.4 to estimate H for this reaction, ignoring the fact that water is in the liquid state.

499

views