![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
thumb_up100%
Calculate the equilibrium constant at 25 °C for each of the following reactions from the value of ΔG° given.
(a) O2(g)+2F2(g)⟶2OF2(g) ΔG°=−9.2 kJ
(b) I2(s)+Br2(l)⟶2IBr(g) ΔG°=7.3 kJ
(c) 2LiOH(s)+CO2(g)⟶Li2CO3(s)+H2O(g) ΔG°=−79 kJ
Expert Solution
![Check Mark](/static/check-mark.png)
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps with 2 images
![Blurred answer](/static/blurred-answer.jpg)
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
- Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) ΔG° = -28.0 kJ P(CO) = 1.4 atm, P(CO2) = 2.1 atmarrow_forwardCalculate ΔGrxn at 298 K under the conditions shown below for the following reaction. Do not enter units with your answer N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔG° = -33.3 kJ P(N2) = 1.0 atm, P(H2) = 3.0 atm, P(NH3) = 9.0 atmarrow_forwardCalculate the equilibrium constant at the temperature given. (Hint: Use formation free energy ΔGf⁰ values to calculate ΔG for the reaction first) (a) I2(s)+Cl2(g)⟶2ICl(g) (T=100°C) (b) H2(g)+I2(s)⟶2HI(g) (T=0.0°C)arrow_forward
- carrow_forwardConsider the following general reaction: A(g) ⇌ B(g) Assuming that the ΔGo for this reaction is +50.2 J/mol, what is the equilibrium constant of this reaction at 420 K? (Please provide your answer to 3 significant figures.)arrow_forward1. Consider the reaction: A 2 B, where Keg 1.33 x 10-1. (a) What is the AGº' for this reaction? (b) If the reaction above is initially at standard-state conditions, what are the concentrations of A and B once equilibrium is reached?arrow_forward
- Kp for the following reaction is 0.16 at 25 0C. 2NOBr(g)=2NO (g)+ Br2 (l) the enthalpy change for the reaction at standard conditions is +16.1 kJ. State which way the equilibrium will shift (left, right or no change) when each of the following changes is made. Breifly explain credit for result. (a) adding more Br2 (l) (b) removing some NOBr (g) (c) Decreasing the temperature (d) increasing the container volume (e) increasing the total pressure by adding an inert gas.arrow_forwardUse the thermodynamic data provided below to determine the ΔGº for the reaction. 1A(s) + 4B(g) -> 1C(s) + 2D(g) Given the following: ΔGf° = -96.0 kJ mol-1 for substance A (s) ΔGfº = 254.0 kJ mol-1 for substance B (g) ΔGfº = 59.0 kJ mol-1 for substance C (s) ΔGfº= 248.0 kJ mol-1 for substance D (g) Provide your answer with final units of kJ and to one decimal place.arrow_forwardThe vapor pressure of solid CO2 (dry ice) is 280. torr at −90. °C and 105 torr at −100. °C. (a) What is the value of ΔG° for the reaction CO2(s) CO2(g) at each temperature? ΔG° at −90 °C 1.52 kJ/mol ΔG° at −100 °C 2.85 kJ/mol (b) What are ΔH° and ΔS° for the reaction CO2(s) CO2(g) at these temperatures? Assume that ΔH° and ΔS° are constant over this temperature range. ΔH° 26 kJ/mol ΔS° J/K·mol need delta S not(c) A dry ice bath is used routinely in the laboratory to keep things cold. It is made by making a power of the dry ice and then mixing the powder with a solvent to make a slurry. Estimate the temperature of the dry ice bath by determining the temperature at which the vapor pressure of CO2 is 1 atm. (only need delta s part and part c please)arrow_forward
- Calculating ΔG under Nonstandard Conditions What is the free energy change for theprocess shown here under the specified conditions? 2NH3(g) ⟶ 3H2(g) + N2(g) ΔG°=33.0 kJ/mol T = 25 °C, PN2 = 0.870 atm, PH2 = 0.250 atm, and PNH3 = 12.9 atmarrow_forwardWhat is the increment G degree for the following reaction from the equilibrium constant at the temperature given? CaCO33(s) → CaO(s) + CO2(g)T = 900°C Kp= 1.04arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
![Text book image](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
![Text book image](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY