Warning: foreach() argument must be of type array|object, bool given in /var/www/html/web/app/themes/studypress-core-theme/template-parts/header/mobile-offcanvas.php on line 20

For which of the following reactions does \(\Delta H_{\mathrm{rxn}}^{\circ}=\Delta H_{\mathrm{f}}^{\circ}\) ? (a) \(\mathrm{H}_{2}(g)+\mathrm{S}(\) rhombic \() \longrightarrow \mathrm{H}_{2} \mathrm{~S}(g)\) (b) \(\mathrm{C}(\) diamond \()+\mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)\) (c) \(\mathrm{H}_{2}(\mathrm{~g})+\mathrm{CuO}(s) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Cu}(s)\) (d) \(\mathrm{O}(g)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{O}_{3}(g)\)

Short Answer

Expert verified
Reaction (a) is the one where \( \Delta H_{\mathrm{rxn}}^{\circ} = \Delta H_{\mathrm{f}}^{\circ} \).

Step by step solution

01

Understand Enthalpy of Formation

The enthalpy of formation, \( \Delta H_{\mathrm{f}}^{\circ} \), is the heat change that results when one mole of a compound is formed from its elements in their standard states. It applies when the products are formed from elements in their most stable form.
02

Analyze Each Reaction

We need to determine if each given reaction represents the formation of one mole of a compound from its elements in their standard states and their most stable forms.
03

Check Reaction (a)

In reaction (a), \( \mathrm{H}_{2}(g)+\mathrm{S}(\text{rhombic}) \rightarrow \mathrm{H}_{2} \mathrm{~S}(g) \), hydrogen gas and rhombic sulfur (standard states) form hydrogen sulfide gas. This fits the criterion for \( \Delta H_{\mathrm{rxn}}^{\circ} = \Delta H_{\mathrm{f}}^{\circ} \).
04

Check Reaction (b)

In reaction (b), \( \mathrm{C}(\text{diamond})+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g) \), carbon as diamond is not in its most stable form (graphite is), thus \( \Delta H_{\mathrm{rxn}}^{\circ} eq \Delta H_{\mathrm{f}}^{\circ} \).
05

Check Reaction (c)

In reaction (c), \( \mathrm{H}_{2}(g)+\mathrm{CuO}(s) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Cu}(s) \), neither \( \mathrm{CuO} \) nor \( \mathrm{H}_{2} \mathrm{O} \) are formed from their most stable elements; \( \Delta H_{\mathrm{rxn}}^{\circ} eq \Delta H_{\mathrm{f}}^{\circ} \).
06

Check Reaction (d)

In reaction (d), \( \mathrm{O}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{O}_{3}(g) \), only ozone \( \mathrm{O}_{3} \) is formed directly from elements, but \( \mathrm{O}(g) \) is not in its most stable form (\( \mathrm{O}_{2}(g) \) is). Hence, \( \Delta H_{\mathrm{rxn}}^{\circ} eq \Delta H_{\mathrm{f}}^{\circ} \).
07

Conclusion

Only reaction (a) follows the conditions for the reaction's enthalpy to equal the enthalpy of formation, as it forms a compound directly from its elements in their standard states.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with Vaia!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Standard States
In the world of chemistry, standard states are crucial for calculations involving thermodynamic quantities like enthalpy, entropy, and Gibbs free energy. A standard state of an element or compound is its most stable form under a set of standard conditions.
Standard conditions are defined as a pressure of 1 bar and a specific temperature, usually 298 K (25°C), although temperature can vary depending on what is being studied. For gases, the standard state is typically 1 bar pressure, for solutes in solution it is 1 M concentration, and for pure substances this means the pure liquid or solid under 1 bar pressure.
  • Gases: 1 bar pressure, often 298 K.
  • Solutions: 1 M concentration.
  • Pure substances: 1 bar pressure in their stable form.
Therefore, a reaction involving elements in their standard states allows for a consistent baseline from which we can compare changes and measure reaction properties, such as enthalpy.
Introduction to Chemical Reactions
Chemical reactions involve the transformation of reactants into products. During this process, chemical bonds break in the reactants and new bonds form in the products. The energy changes associated with these transformations can be calculated in terms of enthalpy changes.
In a balanced chemical equation, the number and type of atoms on both sides of the reaction must be the same, reflecting the law of conservation of mass.
  • Reactants: The starting substances in a chemical reaction.
  • Products: The substances formed from the reaction.
  • Balanced Equation: Same number of each type of atom on either side.
Overall, understanding how atoms rearrange allows chemists to predict how substances will react and what products will form, which is fundamental for controlling reactions in industrial and laboratory settings.
What is Enthalpy?
Enthalpy, represented by the symbol \(H\), is a measure of the total heat content in a chemical system at constant pressure. It encompasses both the internal energy of the system plus the energy required to make room for it (pressure-volume work).
The change in enthalpy (\( \Delta H \)) during a reaction tells us whether a reaction absorbs or releases heat.
  • Exothermic Reaction: \( \Delta H < 0 \), releases heat.
  • Endothermic Reaction: \( \Delta H > 0 \), absorbs heat.
Understanding enthalpy helps in catering industrial processes such as combustion and making energy-efficient systems, by predicting whether a reaction releases or requires energy.
Exploring Heat Change in Reactions
Heat change is a key aspect of chemical reactions, often dictating the feasibility and spontaneity of a process. Heat change in reactions is generally represented by the change in enthalpy (\( \Delta H \)).
For a reaction to have its \( \Delta H_{\text{rxn}}^{\circ} = \Delta H_{\text{f}}^{\circ} \), the reaction should involve the formation of one mole of a substance directly from its constituent elements in their standard states as in reaction (a).
  • Positive \( \Delta H \): Reaction absorbs heat, not favorable without input of energy.
  • Negative \( \Delta H \): Reaction releases heat, often favorable.
Through applying these principles, scientists and engineers can harness chemical reactions for practical applications, like energy production and material synthesis, ensuring the processes are economically and environmentally sustainable.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

A quantity of \(50.0 \mathrm{~mL}\) of \(0.200 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) is mixed with \(50.0 \mathrm{~mL}\) of \(0.400 \mathrm{M} \mathrm{HNO}_{3}\) in a constant-pressure calorimeter having a heat capacity of \(496 \mathrm{~J} /{ }^{\circ} \mathrm{C}\). The initial temperature of both solutions is the same at \(22.4^{\circ} \mathrm{C}\). What is the final temperature of the mixed solution? Assume that the specific heat of the solutions is the same as that of water and the molar heat of neutralization is \(-56.2 \mathrm{~kJ} / \mathrm{mol}\).

The standard enthalpies of formation of ions in aqueous solutions are obtained by arbitrarily assigning a value of zero to \(\mathrm{H}^{+}\) ions; that is, \(\Delta H_{\mathrm{f}}^{\mathrm{o}}\left[\mathrm{H}^{+}(a q)\right]=0 .\) (a) For the following reaction \(\begin{aligned} \mathrm{HCl}(g) \stackrel{\mathrm{H}_{2} \mathrm{O}}{\longrightarrow} \mathrm{H}^{+}(a q)+\mathrm{Cl}^{-}(a q) & \Delta H^{\circ}=-74.9 \mathrm{~kJ} / \mathrm{mol} \end{aligned}\) calculate \(\Delta H_{\mathrm{f}}^{\circ}\) for the \(\mathrm{Cl}^{-}\) ions. \((\mathrm{b})\) Given that \(\Delta H_{\mathrm{f}}^{\circ}\) for \(\mathrm{OH}^{-}\) ions is \(-229.6 \mathrm{~kJ} / \mathrm{mol},\) calculate the enthalpy of neutralization when 1 mole of a strong monoprotic acid (such as \(\mathrm{HCl}\) ) is titrated by \(1 \mathrm{~mole}\) of a strong base \((\) such as \(\mathrm{KOH})\) at \(25^{\circ} \mathrm{C}\).

A student mixes \(88.6 \mathrm{~g}\) of water at \(74.3^{\circ} \mathrm{C}\) with \(57.9 \mathrm{~g}\) of water at \(24.8^{\circ} \mathrm{C}\) in an insulated flask. What is the final temperature of the combined water?

Define calorimetry and describe two commonly used calorimeters. In a calorimetric measurement, why is it important that we know the heat capacity of the calorimeter? How is this value determined?

Consider two metals A and B, each having a mass of \(100 \mathrm{~g}\) and an initial temperature of \(20^{\circ} \mathrm{C}\). The specific heat of \(\mathrm{A}\) is larger than that of \(\mathrm{B}\). Under the same heating conditions, which metal would take longer to reach a temperature of \(21^{\circ} \mathrm{C} ?\)

See all solutions

Recommended explanations on Chemistry Textbooks

View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free