Modified Mastering Chemistry with Pearson eText -- Standalone Access Card -- for General, Organic, and Biological Chemistry (3rd Edition)
3rd Edition
ISBN: 9780134143705
Author: Laura D. Frost, S. Todd Deal
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 5, Problem 5.2PP
In your own words, define free energy change, ΔG.
- a. How does the ΔG differ in exergonic and endergonic reactions?
- b. Which is spontaneous, a reaction with a + or − value for ΔG?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Can someone draw an energy Diagram with the following:
The reaction is not spontaneous, the first step is exergonic and slow, the reaction has a total of three steps, the second step is a slow equilibrium, and the third step is faster than the first
And how would I go about taking this information and drawing a energy diagram? 
Experimental observations of a biochemical reaction have indicated that the reaction releases free energy to its surroundings. What is the name for this type of reaction and what sign is associated with its value for change of free energy?
a. Exothermic, negative
b. Exothermic, positive
c. Endothermic, negative
d. Exergonic, negative
e. Endothermic, positive
The standard reaction free energy AG°
= - 190. kJ for this reaction:
CH3OH(g) + CO(g) -»HCH3CO2(l)
Use this information to complete the table below. Round each of your answers to the nearest kJ.
Chapter 5 Solutions
Modified Mastering Chemistry with Pearson eText -- Standalone Access Card -- for General, Organic, and Biological Chemistry (3rd Edition)
Ch. 5 - When vinegar (CH3COOH) and baking soda (NaHCO3)...Ch. 5 - In your own words, define free energy change, G....Ch. 5 - Classify the following as exothermic or...Ch. 5 - Prob. 5.4PPCh. 5 - Prob. 5.5PPCh. 5 - Classify the following as spontaneous or...Ch. 5 - Prob. 5.7PPCh. 5 - Prob. 5.8PPCh. 5 - Prob. 5.9PPCh. 5 - Prob. 5.10PP
Ch. 5 - a. How does increasing the temperature increase...Ch. 5 - a. Describe activation energy for a chemical...Ch. 5 - Why does the rate of a chemical reaction decrease...Ch. 5 - Prob. 5.14PPCh. 5 - Enzymes increase the rate of a biological chemical...Ch. 5 - Prob. 5.16PPCh. 5 - Prob. 5.17PPCh. 5 - Prob. 5.18PPCh. 5 - Categorize the following reactions as synthesis,...Ch. 5 - Categorize the following reactions as synthesis,...Ch. 5 - Prob. 5.21PPCh. 5 - Prob. 5.22PPCh. 5 - Write the products and balance the following...Ch. 5 - Prob. 5.24PPCh. 5 - Prob. 5.25PPCh. 5 - List the differences between general chemical...Ch. 5 - Are the substances shown in italics undergoing...Ch. 5 - Prob. 5.28PPCh. 5 - Prob. 5.29PPCh. 5 - Prob. 5.30PPCh. 5 - Prob. 5.31PPCh. 5 - Prob. 5.32PPCh. 5 - Prob. 5.33PPCh. 5 - Prob. 5.34PPCh. 5 - Prob. 5.35PPCh. 5 - Prob. 5.36PPCh. 5 - Prob. 5.37PPCh. 5 - Write the main product of hydration for the...Ch. 5 - Methane (a.k.a. natural gas) can react with oxygen...Ch. 5 - Prob. 5.40APCh. 5 - Which reaction occurs at a faster rate, an...Ch. 5 - Prob. 5.42APCh. 5 - Prob. 5.43APCh. 5 - Two curves for the same reaction are shown in the...Ch. 5 - Prob. 5.45APCh. 5 - Draw and label a reaction energy diagram for an...Ch. 5 - Prob. 5.47APCh. 5 - Prob. 5.48APCh. 5 - Write the products that would result from the...Ch. 5 - Prob. 5.50APCh. 5 - Prob. 5.51APCh. 5 - Prob. 5.52APCh. 5 - Prob. 5.53APCh. 5 - Prob. 5.54APCh. 5 - Prob. 5.55APCh. 5 - Identify the reactant that is oxidized and the...Ch. 5 - Prob. 5.57APCh. 5 - Write the products of the following reactions:Ch. 5 - Prob. 5.59APCh. 5 - Acetylsalicylic acid (aspirin) can be synthesized...Ch. 5 - Prob. 5.61APCh. 5 - Fill in the missing organic produce for the...Ch. 5 - Prob. 5.63APCh. 5 - Prob. 5.64APCh. 5 - How do low-carb diets work? We store glucose...Ch. 5 - Prob. 5.66CPCh. 5 - Prob. 5.67CPCh. 5 - Prob. 5.68CPCh. 5 - Prob. 5.69CPCh. 5 - Which reaction has the larger activation energy?Ch. 5 - Prob. 1IA.2QCh. 5 - A catalyst speeds up a chemical reaction by...Ch. 5 - Prob. 1IA.4QCh. 5 - Examine your sketch from question 3. Does a...Ch. 5 - Prob. 1IA.6QCh. 5 - Prob. 2IA.1QCh. 5 - Prob. 2IA.2QCh. 5 - Prob. 2IA.3QCh. 5 - One of the reactions in the data set is a single...Ch. 5 - Prob. 2IA.5QCh. 5 - Categorize the following reactions as a synthesis,...Ch. 5 - Prob. 3IA.1QCh. 5 - Prob. 3IA.2QCh. 5 - Prob. 3IA.3QCh. 5 - Prob. 3IA.4QCh. 5 - Prob. 3IA.5QCh. 5 - Prob. 1ICCh. 5 - Find out how unsaturated fats are saturated and...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- The molecular scale pictures below show snapshots of a strong acid at three different instants after it is added to water. Place the three pictures in the correct order so that they show the progress of the spontaneous process that takes place as the acid dissolves in the water. Explain your answer in terms of entropyarrow_forwardThe diagram shows the free energy change of the reaction A(g)+B(g)↽−−⇀AB(g) The reaction progress starts on the left with pure reactants, A and B, each at 1 atm, and moves to pure product, AB, which is at 1 atm on the right. Select the true statementsarrow_forwardA negative sign for Δ G indicates that, at constant T and P, Select one: a. the reaction is endothermic. b. the reaction is fast. c. the reaction is spontaneous. d. the reaction is exothermic. e. the reaction is not spontaneous.arrow_forward
- ) A chemical reaction that has a positive Δ G is correctly described as A) endergonic. B) endothermic. C) enthalpic. D) spontaneous. E) exothermic.arrow_forwardTRUE OR FALSE? 1. Entropy changes cannot be measured with a calorimeter like enthalpy changes. 2. If the result upon calculation of entropy changes in the universe is a positive value, the process is reactant-favored. 3. If the change in free energy, ΔG is negative, the reaction is spontaneous in the forward direction.arrow_forwardConsider the ideal combustion of ethanol: C2H5OH(ℓ) + 3 O2(g) → 2 CO2(g) + 3 H2O(ℓ) ∆Ho = -1367.5 molar masses (g/mol): C2H5OH - 46.07 CO2 - 44.01 Indicate the 3 statements about the ideal combustion of ethanol that are true by checking the box in front of each true statement. The reaction is endothermic. The reaction is exothermic. There is more chemical energy stored in the products than in the reactants. When 50.0 g of ethanol combusts, 47.8 g of carbon dioxide are formed. When 50.0 g of ethanol combusts, 1480 kJ are released. When 1030 kJ are released, 40.7 g of water are formed.arrow_forward
- cells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be written as ATP(aq) + H2O(l)--> ADP(aq) + H2PO4-(aq). where ADP represent adenosine diphosphate. For this reaction, ΔG∘=-30.5kj/mol. a. If all the free energy from the metabolism of glucose goes into forming ATP from ADP, how many ATP molecules can be produced for every molecule of glucose? C6H12O6 + 6O2 → 6CO2 + 6H2Oarrow_forwardThe standard free energy change for the reaction CH4(g)+2O2(g) -> CO2(g) + 2H2O(l) is -194.8 kcal at 25ºC and -191.82 kcal at 75ºC. Calculate the heat of reaction at 25ºC.Ans: -212.6 kcalarrow_forwardThe standard reaction free energy AG°=-800. kJ for this reaction: CH4(g) + 2O2(g)>CO2(g) + 2H2O(g) Use this information to complete the table below. Round each of your answers to the nearest kJ.arrow_forward
- 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.arrow_forward∆Gº for the reaction, 2HBr(g)⇄ H2(g)+Br2(g), is 33.3 kJ. Which statement below is true? This reaction must be very fast. This reaction must be very slow. This reaction is spontaneous for these conditions. This reaction is non-spontaneous under these conditions. Question 12 of 15arrow_forwardCalculate the standard free energy for the reaction given. 2 CH 3OH( l) + 3 O 2( g) → 2 CO 2( g) + 4 H 2O( l) a -797.8 kJ b -2069.8 kJ c -1404.8 kJ d -465.2 kJarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
Chemistry for Today: General, Organic, and Bioche...
Chemistry
ISBN:9781305960060
Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY