
(a)
Interpretation:
The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.
Concept Introduction:
Le Chatelier’s principle:
Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium. It is used to understand the conditions of a reaction which favours increased product formation.
The reactions of heat are of two types:
- 1. Exothermic reaction – releases heat
- 2. Endothermic reaction – absorbs heat
Change in equilibrium due to temperature changes:
If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.
If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.
(b)
Interpretation:
The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.
Concept Introduction:
Le Chatelier’s principle:
Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium. It is used to understand the conditions of a reaction which favours increased product formation.
The reactions of heat are of two types:
- 1. Exothermic reaction – releases heat
- 2. Endothermic reaction – absorbs heat
Change in equilibrium due to temperature changes:
If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.
If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.
(c)
Interpretation:
The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.
Concept Introduction:
Le Chatelier’s principle:
Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium. It is used to understand the conditions of a reaction which favours increased product formation.
The reactions of heat are of two types:
- 1. Exothermic reaction – releases heat
- 2. Endothermic reaction – absorbs heat
Change in equilibrium due to temperature changes:
If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.
If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.
(d)
Interpretation:
The effect of increase in the temperature has to be predicted on the amount of products formed in the given reaction.
Concept Introduction:
Le Chatelier’s principle:
Le Chatelier’s principle states that the changes in the temperature, pressure, volume and concentration of the system results in the change in system to attain new equilibrium. It is used to understand the conditions of a reaction which favours increased product formation.
The reactions of heat are of two types:
- 1. Exothermic reaction – releases heat
- 2. Endothermic reaction – absorbs heat
Change in equilibrium due to temperature changes:
If the temperature is increased for the system, the equilibrium shifts away from the heat because of the reaction needs extra heat to use.
If the temperature is decreased for the system, the equilibrium shifts towards the heat because the heat needs to be produced to make up for the loss.

Want to see the full answer?
Check out a sample textbook solution
Chapter 17 Solutions
Loose Leaf for Chemistry: The Molecular Nature of Matter and Change
- Identify and provide an explanation that distinguishes a qualitative and quantitative chemical analysis. Provide examples.arrow_forwardIdentify and provide an explanation of the operational principles behind a Atomic Absorption Spectrometer (AAS). List the steps involved.arrow_forwardInstructions: Complete the questions in the space provided. Show all your work 1. You are trying to determine the rate law expression for a reaction that you are completing at 25°C. You measure the initial reaction rate and the starting concentrations of the reactions for 4 trials. BrO³¯ (aq) + 5Br¯ (aq) + 6H* (aq) → 3Br₂ (l) + 3H2O (l) Initial rate Trial [BrO3] [H*] [Br] (mol/L) (mol/L) | (mol/L) (mol/L.s) 1 0.10 0.10 0.10 8.0 2 0.20 0.10 0.10 16 3 0.10 0.20 0.10 16 4 0.10 0.10 0.20 32 a. Based on the above data what is the rate law expression? b. Solve for the value of k (make sure to include proper units) 2. The proposed reaction mechanism is as follows: i. ii. BrО¸¯ (aq) + H+ (aq) → HBrO3 (aq) HBrO³ (aq) + H* (aq) → H₂BrO3* (aq) iii. H₂BrO³* (aq) + Br¯ (aq) → Br₂O₂ (aq) + H2O (l) [Fast] [Medium] [Slow] iv. Br₂O₂ (aq) + 4H*(aq) + 4Br(aq) → 3Br₂ (l) + H2O (l) [Fast] Evaluate the validity of this proposed reaction. Justify your answer.arrow_forward
- a. H3C CH3 H, 1.0 equiv. Br2arrow_forwardH3C. H3C CH 3 CH 3 CH3 1. LDA 2. PhSeCl 3. H2O2arrow_forwardPlease predict the products for each of the following reactions: 1.03 2. H₂O NaNH, 1. n-BuLi 2. Mel A H₂ 10 9 0 H2SO4, H₂O HgSO4 Pd or Pt (catalyst) B 9 2 n-BuLi ♡ D2 (deuterium) Lindlar's Catalyst 1. NaNH2 2. EtBr Na, ND3 (deuterium) 2. H₂O2, NaOH 1. (Sia)2BH с Darrow_forward
- in the scope of ontario SCH4U grade 12 course, please show ALL workarrow_forwardIs the chemical reaction CuCl42-(green) + 4H2O <==> Cu(H2O)42+(blue) + 4Cl- exothermic or endothermic?arrow_forwardIf we react tetraethoxypropane with hydrazine, what is the product obtained (explain its formula). State the reason why the corresponding dialdehyde is not used.arrow_forward
- 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





