Ch.9 - Thermochemistry: Chemical Energy

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.9 - Thermochemistry: Chemical Energy

Problem 153b

Chapter 9, Problem 153b

(b) Use the data in Appendix B to calculate ΔH° for the reaction of potassium metal with water.

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Identify the balanced chemical equation for the reaction of potassium metal with water. The reaction is typically: \(2K(s) + 2H_2O(l) \rightarrow 2KOH(aq) + H_2(g)\).

Look up the standard enthalpy of formation (\(\Delta H_f^\circ\)) values for each reactant and product in the reaction from Appendix B. You will need the values for \(K(s)\), \(H_2O(l)\), \(KOH(aq)\), and \(H_2(g)\).

Apply Hess's Law which states that the total enthalpy change for a reaction is the sum of the enthalpy changes for each step of the reaction, regardless of the path taken. For this reaction, calculate \(\Delta H^\circ_{reaction}\) using the formula: \(\Delta H^\circ_{reaction} = \sum (\Delta H_f^\circ \text{ of products}) - \sum (\Delta H_f^\circ \text{ of reactants})\).

Multiply the \(\Delta H_f^\circ\) of each substance by its respective coefficient in the balanced chemical equation.

Sum up all the values obtained in the previous step to find the total \(\Delta H^\circ_{reaction}\) for the reaction of potassium metal with water.

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Key Concepts

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

Enthalpy Change (ΔH°)

Enthalpy change, denoted as ΔH°, refers to the heat content change of a system at constant pressure during a chemical reaction. It indicates whether a reaction is exothermic (releases heat, ΔH° < 0) or endothermic (absorbs heat, ΔH° > 0). Understanding how to calculate ΔH° is crucial for predicting the energy changes associated with chemical reactions.

Standard State Conditions

Standard state conditions refer to the specific set of conditions (1 atm pressure, 25°C temperature) under which the standard enthalpy of formation and other thermodynamic properties are measured. These conditions provide a reference point for comparing the enthalpy changes of different reactions, ensuring consistency in calculations and interpretations.

Hess's Law

Hess's Law states that the total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps of the reaction, regardless of the pathway taken. This principle allows chemists to calculate ΔH° for complex reactions by using known enthalpy values from simpler reactions, facilitating the determination of energy changes in multi-step processes.

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Hess's Law

Related Practice

Textbook Question

Acid spills are often neutralized with sodium carbonate or sodium hydrogen carbonate. For neutralization of acetic acid, the unbalanced equations are

(1) CH₃CO₂H(l) + Na₂CO₃(s) → CH₃CO₂Na(aq) + CO₂(g) + H₂O(l)

(2) CH₃CO₂H(l) + NaHCO₃(s) → CH₃CO₂Na(aq) + CO₂(g) + H₂O(l)

(a) Balance both equations.

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Textbook Question

Acid spills are often neutralized with sodium carbonate or sodium hydrogen carbonate. For neutralization of acetic acid, the unbalanced equations are

(1) CH₃CO₂H(l) + Na₂CO₃(s) → CH₃CO₂Na(aq) + CO₂(g) + H₂O(l)

(2) CH₃CO₂H(l) + NaHCO₃(s) → CH₃CO₂Na(aq) + CO₂(g) + H₂O(l)

(b) How many kilograms of each substance is needed to neutralize a 1.000-gallon spill of pure acetic acid (density = 1.049 g/mL)?

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Textbook Question

(d) What is the molarity of the KOH solution prepared in part (c), and how many milliliters of 0.554 M H2SO4 are required to neutralize it?

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Textbook Question

Reaction of gaseous fluorine with compound X yields a single product Y, whose mass percent composition is 61.7% F and 38.3% Cl. (a) What is a probable molecular formula for product Y, and what is a probable formula for X?

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Textbook Question

Acid spills are often neutralized with sodium carbonate or sodium hydrogen carbonate. For neutralization of acetic acid, the unbalanced equations are112 CH3CO2H1l2 + Na2CO31s2 SCH3CO2Na1aq2 + CO21g2 + H2O1l2 122 CH3CO2H1l2 + NaHCO31s2CH3CO2Na1aq2 + CO21g2 + H2O1l2(c) How much heat in kilojoules is absorbed or liberated in each reaction? See Appendix B for standard heats of for- mation; ΔH°f = - 726.1 kJ>mol for CH3CO2 Na(aq).

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Textbook Question

(c) Assume that a chunk of potassium weighing 7.55 g is dropped into 400.0 g of water at 25.0 °C. What is the final temperature of the water if all the heat released is used to warm the water?

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