Ch. 17 - Chemical ThermodynamicsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: A particular chemical reaction has a negative ΔH and a negative ΔS. Which statement is correct?(A) The reaction is spontaneous at all temperatures.(B) The reaction is non spontaneous at all temperatur

Solution: A particular chemical reaction has a negative ΔH and a negative ΔS. Which statement is correct?(A) The reaction is spontaneous at all temperatures.(B) The reaction is non spontaneous at all temperatur

Problem

A particular chemical reaction has a negative ΔH and a negative ΔS. Which statement is correct?

(A) The reaction is spontaneous at all temperatures.

(B) The reaction is non spontaneous at all temperatures.

(C) The reaction becomes spontaneous as temperature increases.

(D) The reaction becomes spontaneous as temperature decreases.

Solution

We’re being asked to determine which of the given statements is correct for a reaction given the sign of its ΔH and  ΔS.


The statements given describe the spontaneity of the reaction at different temperatures

Recall that when ΔH and ΔS are given, we can determine the spontaneity of the reaction based on their signs

We can use the Punnett square shown below:

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