Which of the following processes are spontaneous and which are nonspontaneous: (e) formation of CH 4 and O 2 molecules from CO 2 and H 2 O at room temperature and 1 atm of pressure?

Hello, everyone in this video, We're trying to see if this following statement is true or false. The statement reads the reaction of N two gas and C. 02 gas occurs spontaneously to produce gas, and so gas at room temperature and standard pressure conditions of one atmosphere. So let's see here, we know that our N to N C. 02 are always intact and normal standard atmospheric conditions, but the products that they're talking about, which is N. O. Gas and so gas will not form spontaneously without any sort of intervention. Therefore, the statement then is false. So the false is going to be my final answer for this. Thank you all so much for watching.

Ch.19 - Chemical Thermodynamics

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Brown 14th Edition

Ch.19 - Chemical Thermodynamics

Problem 11e

Chapter 19, Problem 11e

Which of the following processes are spontaneous and which are nonspontaneous: (e) formation of CH₄ and O₂ molecules from CO₂ and H₂O at room temperature and 1 atm of pressure?

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Understand the concept of spontaneity: A spontaneous process is one that occurs without needing to be driven by an external force. It is often associated with a decrease in free energy (ΔG < 0).

Identify the chemical reaction: The formation of CH₄ and O₂ from CO₂ and H₂O can be represented as: CO₂ + 2H₂O → CH₄ + 2O₂.

Consider the thermodynamics: Determine if the reaction is exothermic or endothermic by considering the enthalpy change (ΔH). Formation of CH₄ and O₂ from CO₂ and H₂O is typically endothermic, requiring energy input.

Evaluate the entropy change (ΔS): Consider the change in disorder. The reaction involves breaking stable CO₂ and H₂O molecules to form CH₄ and O₂, which may decrease entropy.

Apply Gibbs Free Energy equation: Use ΔG = ΔH - TΔS to assess spontaneity. If ΔG is positive, the process is nonspontaneous under the given conditions (room temperature and 1 atm).

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Key Concepts

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

Spontaneity of Reactions

A spontaneous process is one that occurs without needing to be driven by an external force. In thermodynamics, spontaneity is often determined by the change in Gibbs free energy (ΔG); if ΔG is negative, the process is spontaneous. This concept is crucial for understanding whether a reaction will proceed under given conditions.

Gibbs Free Energy

Gibbs free energy is a thermodynamic potential that measures the maximum reversible work obtainable from a thermodynamic system at constant temperature and pressure. The equation ΔG = ΔH - TΔS relates changes in enthalpy (ΔH) and entropy (ΔS) to spontaneity. A negative ΔG indicates that the reaction can occur spontaneously.

Standard Conditions

Standard conditions refer to a set of specific conditions (usually 1 atm pressure and a specified temperature, often 25°C) under which thermodynamic data is tabulated. These conditions are essential for comparing the spontaneity of reactions, as they provide a consistent reference point for calculating Gibbs free energy and other thermodynamic properties.

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Which of the following processes are spontaneous and which are nonspontaneous: (a) the ripening of a banana

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Textbook Question

Which of the following processes are spontaneous and which are nonspontaneous: (d) lightning

Which of the following processes are spontaneous?

a. the melting of ice cubes at −10 °C and 1 atm pressure

b. separating a mixture of N₂ and O₂ into two separate samples, one that is pure N₂ and one that is pure O₂

c. alignment of iron filings in a magnetic field

d. the reaction of hydrogen gas with oxygen gas to form water vapor at room temperature

e. the dissolution of HCl(g) in water to form concentrated hydrochloric acid

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Textbook Question

Indicate whether each statement is true or false. (a) A reaction that is spontaneous in one direction will be nonspontaneous in the reverse direction under the same reaction conditions. (b) All spontaneous processes are fast. (c) Most spontaneous processes are reversible. (d) An isothermal process is one in which the system loses no heat. (e) The maximum amount of work can be accomplished by an irreversible process rather than a reversible one.

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Which of the following processes are spontaneous and which are nonspontaneous: (e) formation of CH4 and O2 molecules from CO2 and H2O at room temperature and 1 atm of pressure?

Verified video answer for a similar problem:

Key Concepts

Spontaneity of Reactions

Gibbs Free Energy

Standard Conditions

Which of the following processes are spontaneous and which are nonspontaneous: (e) formation of CH₄ and O₂ molecules from CO₂ and H₂O at room temperature and 1 atm of pressure?