(a)
Interpretation:
The effect on the equilibrium concentration of
Concept Introduction:
Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.
Factor’s that effect chemical equilibria:
- Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.
- Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.
- Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.
If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.
(b)
Interpretation:
The effect on the equilibrium concentration of
Concept Introduction:
Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.
Factor’s that effect chemical equilibria:
- Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.
- Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.
- Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.
If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.
(c)
Interpretation:
The effect on the equilibrium concentration of
Concept Introduction:
Enthalpy
If the value obtained for
Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.
Factor’s that effect chemical equilibria:
- Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.
- Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.
- Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.
If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.
(d)
Interpretation:
The effect on the equilibrium concentration of
Concept Introduction:
Le Chatelier’s principle: If an equilibrium is disturbed by changing conditions, the system will moves the equilibrium to reverse the change.
Factor’s that effect chemical equilibria:
- Concentration – Equilibrium will be affected by changing the concentration of reactant or product. If we increase the concentration of reactant system will try to reverse the change by favouring forward reaction and thus increase the concentration of products. Likewise adding products increase yield of reactants.
- Temperature – When the temperature increases equilibrium will shift in the endothermic direction, in the direction that absorbs heat. When the temperature decreases equilibrium will shift in the exothermic direction, in the direction that releases heat.
- Pressure – If the reaction consists of only liquid and solid reactants and products, pressure has no effect in the equilibrium.
In gas reactions if the number of moles has no change then there will be no effect by pressure on equilibrium.
If pressure increases then equilibrium will shift to the direction having less number of molecules and if pressure decreases system will shift to the direction having more number of molecules.
Catalyst: Substance which helps in increasing the rate of a particular reaction without getting consumed in the reaction.
Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo
Want to see the full answer?
Check out a sample textbook solutionChapter 7 Solutions
EBK FUNDAMENTALS OF GENERAL, ORGANIC, A
- Potassium superoxide, KO2, is used in rebreathing masks to generate oxygen according to the reaction below. If the mask contains 0.250 mol KO2 and 0.200 mol water, what is the limiting reagent? How many moles of excess reactant will there be once the reaction is complete? 4 KO2(s) + 2 H2O(ℓ) → 4 KOH(s) + 3 O2(g)arrow_forwardComplete the following precipitation reactions using balanced chemical equations:arrow_forwardThe following questions are based on the reaction A+ B ↔ C+D shown in Figure 8.1. 1. Which of the following terms best describes the progress of the reaction with respect to free energy change? a) endergonic, ∆G> 0 b) exergonic, ∆G> 0 c) exergonic, ∆G< 0 d) endergonic, ∆G< 0 2. Which of the following in Figure 8.1 remains unchanged by having an enzyme included? a) b b) d c) a d) c 3. The part labeled “C” on the above graph represents a) Energy of activation without enzyme b) Energy of activation with enzyme c) Amount of free energy released d) amount of energy required for the reaction progressarrow_forward
- How will each change affect the reaction? HNO2(aq)⇌H^+(aq)+NO2^-(aq) a.) Decreasing volume b.) Removal of NO2^- c.) Addition of OH^-(which will react with and remove H^+)arrow_forwardCarboxylic acids, such as the one shown below, can be difficult to reduce Provide the name of a reductant A. Explain why this reductant is able to react with the carboxylic acid whereas others cannot (Hint: Draw and discuss the potential reactive intermediates/transition states).arrow_forwardNutritional biochemists have known for decades that acidicfoods cooked in cast-iron cookware can supply significantamounts of dietary iron (ferrous ion).(a) Write a balanced net ionic equation, with oxidation numbers,that supports this fact.(b) Measurements show an increase from 3.3 mg of iron to49 mg of iron per 1/2 -cup (125-g) serving during the slow prepa-ration of tomato sauce in a cast-iron pot. How many ferrous ionsare present in a 26-oz (737-g) jar of the tomato sauce?arrow_forward
- In another key reaction in glycolysis, dihydroxyacetone phosphate (DHAP) is isomerized into glyceraldehyde-3-phosphate (GAP): CH,OH | C=0 НС — ОН AG" = +7.5 kJ/mol CH,OPO,?- CH,OPO,- DHAP GAP Because AG° is positive, the equilibrium lies to the left. (a) Calculate the equilibrium constant, and the equilibrium fraction of GAP from the above, at 37 °C. (b) In the cell, depletion of GAP makes the reaction proceed. What will AG be if the concentration of GAP is always kept at 1/100 of the concentration of DHAP?arrow_forwardIdentify the oxidized reactant, the reduced reactant, the oxidizing agent, and the reducing agent in the following reactions:arrow_forwardI Write a balanced equation for each of the following two reactions that you will use in this activity. In the boxes provided, draw a diagram showing this reaction at the molecular level. Be sure that the drawing shows conservation of mass (see Figure 1.7A and B). a Calcium chloride reacting with sodium phosphate (double replacement) CaCl2 (aq) + NazPO4 (aq) → (_) + Reactants Products b Zinc reacting with hydrochloric acid (single replacement) Zn (s) + HCI (aq) → (_) + Reactants Productsarrow_forward
- Calculate the equilibrium constant for the reaction glucose-1-phosphate + H2O → glucose + H2PO4− at pH 7.0 and 25°C (ΔG°′ = −20.9 kJ · mol−1).arrow_forwardConsider the following reaction: Glucose-1-phosphate → Glucose-6-phosphate ΔG° = −7.1 kJ/mol What is the equilibrium constant for this reaction at 25oC?arrow_forwardWhich of these condition of all substrates and en standard state of a biological system? a) There is a 1M enzymes. b) There is a 1M concentration of H+. a) c) The solution is at 25°C. It is assumed the activity of 55M H₂O is the same as the activity at IM H₂O. 2. What is the AG of a reaction at equilibrium? a) AG 0 d) Equilibrium and AG are not related CXWhich of the following is an omega-6 fatty acid? b) CHow are solid fats and oils different? a) fats contain triacylglycerols with more double bonds than oils. b) fats contain triacylglycerols with three fatty acid chains while oils have triacylglycerols with two fatty acid chains. OH d) c) fats contain triacylglycerols and oils contain fatty acids d) fats contain triacylglycerols with fewer double bonds than oil OH OHarrow_forward
- BiochemistryBiochemistryISBN:9781319114671Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.Publisher:W. H. FreemanLehninger Principles of BiochemistryBiochemistryISBN:9781464126116Author:David L. Nelson, Michael M. CoxPublisher:W. H. FreemanFundamentals of Biochemistry: Life at the Molecul...BiochemistryISBN:9781118918401Author:Donald Voet, Judith G. Voet, Charlotte W. PrattPublisher:WILEY
- BiochemistryBiochemistryISBN:9781305961135Author:Mary K. Campbell, Shawn O. Farrell, Owen M. McDougalPublisher:Cengage LearningBiochemistryBiochemistryISBN:9781305577206Author:Reginald H. Garrett, Charles M. GrishamPublisher:Cengage LearningFundamentals of General, Organic, and Biological ...BiochemistryISBN:9780134015187Author:John E. McMurry, David S. Ballantine, Carl A. Hoeger, Virginia E. PetersonPublisher:PEARSON