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
Related questions
Question
![### Chemical Equilibrium and Reaction Effects
#### Question 261
Hydrogen, bromine, and HBr in the gas phase are in equilibrium in a container of fixed volume.
\[ \text{H}_2(g) + \text{Br}_2(g) \rightleftharpoons 2 \text{HBr}(g) \, \, (\text{+ heat}) \quad \Delta H^\circ = -103.7 \, \text{kJ} \]
**How will each of the following changes affect the equilibrium and the value of the equilibrium constant?**
a) Some \(\text{H}_2(g)\) is added to the container.
b) The pressure of \(\text{HBr}(g)\) is increased.
c) The temperature of this system is increased.
#### Question 262
Predict the effect on this reaction if the following changes are made.
\[ \text{Fe(OH)}_3(s) + \text{H}_2\text{O}(l) \rightarrow \text{Fe}^{3+}(aq) + 3 \text{OH}^-(aq) \]
a) \(\text{Fe(NO}_3)_3(aq)\) is added:
b) \(\text{NaOH}(aq)\) is added:
c) \(\text{Fe(OH)}_3(s)\) is added:
d) \(\text{HCl}(aq)\) is added:](https://content.bartleby.com/qna-images/question/d7f1690c-47e2-42cd-b38b-5e904dfd21d9/6d33ff9a-b0b8-4396-8480-e6faf9e6bd8c/6gmcip_processed.jpeg)
Transcribed Image Text:### Chemical Equilibrium and Reaction Effects
#### Question 261
Hydrogen, bromine, and HBr in the gas phase are in equilibrium in a container of fixed volume.
\[ \text{H}_2(g) + \text{Br}_2(g) \rightleftharpoons 2 \text{HBr}(g) \, \, (\text{+ heat}) \quad \Delta H^\circ = -103.7 \, \text{kJ} \]
**How will each of the following changes affect the equilibrium and the value of the equilibrium constant?**
a) Some \(\text{H}_2(g)\) is added to the container.
b) The pressure of \(\text{HBr}(g)\) is increased.
c) The temperature of this system is increased.
#### Question 262
Predict the effect on this reaction if the following changes are made.
\[ \text{Fe(OH)}_3(s) + \text{H}_2\text{O}(l) \rightarrow \text{Fe}^{3+}(aq) + 3 \text{OH}^-(aq) \]
a) \(\text{Fe(NO}_3)_3(aq)\) is added:
b) \(\text{NaOH}(aq)\) is added:
c) \(\text{Fe(OH)}_3(s)\) is added:
d) \(\text{HCl}(aq)\) is added:
Expert Solution
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
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
- Given the equation 2A(g) 2B(g) + C(g). At a particular temperature, K = 1.6 × 104.Addition of chemical B to an equilibrium mixture of the above will a cause [A] to increase b cause [C] to increase c have no effect d cannot be determined e none of the abovearrow_forwardFor the reaction PCl3 (g) + Cl2 (g) → PCl5 (g)A system starts with 0.760 atm of PCl3 and 0.590 atm of Cl2 at 401.4 K.At equilibrium, the final pressure of PCl5 is 0.453 atm.a) What is the equilibrium constant, KP, for this reaction?arrow_forwardConsider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. KJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? rise ☐ x10 fall оо Is it possible to reverse this tendency by adding H₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ at atmarrow_forward
- Consider the following chemical equilibrium: 2 A2 (g) 2 B (g) + C (g) Kp = 1.2 x 103 What would happen if the volume of its container was lowered at constant temperature? O A. We would need to know whether the reaction is exothermic or endothermic to predict O B. The equilibrium constant would increase O C. The amount of A2 would increase O D. No change would happen O E. The amount of A2 would decrease Reset Selectionarrow_forwardDarrow_forwardConsider the reaction. 2 A(g) = B(g) Kp = 5.78 × 10-5 If a sample of A(g) at 1.50 atm is heated to 500 K, what is the pressure of B(g) at equilibrium? PB || at 500 K atmarrow_forward
- Consider the following reaction: COCI,(g) CO(g) + Cl(g) If 1.39×102 moles of COCl,, 0.302 moles of CO, and 0.244 moles of Cl, are at equilibrium in a 13.2 L container at 720 K, the value of the equilibrium constant, Kp. isarrow_forwardFor the following reaction H₂(g) + ₂(g) → 2HI(g) 2 AH° = -10.64 kJ/mol and AS° = 21.48 J/mol K. A closed container in which P_H₂ = P_I₂ = 0.100 atm and P_HI = 0.500 atm is heated to 555 °C at constant pressure. After equilibrium is attained at that temperature, what is the pressure of HI in atm? Assume AH° and AS° are temperature independent.arrow_forward29. Consider the following equilibrium process at 700°C: 2 H2 (g) + S2 (g) → 2 H2S (g). Analysis at equilibrium shows that there are 2.5 moles of H2, 1.35 x 10-5 moles of S2 and 8.70 moles of H2S present in a 12.0 liter flask. Calculate the equilibrium constant Ke for the reaction. K.arrow_forward
- 4.arrow_forwardHelp with the following question. Please round the answer to 2 decimal places arrow_forwardFor the reaction CaO(s) + CO2(g) CaCO3(s), the value of AH is -178 kJ/mol. Using Le Chatelier's principle, which of the following changes to the system will shift the equilibrium to the right? i) Increasing the amount of CaO. ii) Decreasing the volume of the container. iii) Increasing the temperature. iv) Decreasing the temperature O A. only ii and iii OB. only i & ii OC. all of them OD. only i & iv OE. only i & iiiarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles 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 Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY