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a.
To classify:
The given reaction as exothermic or endothermic.
Introduction:
The equilibrium constant is a parameter which describes the relationship between the concentration of the reactants and the products at equilibrium stage. The equilibrium constant of a reaction is expressed by the ratio of the concentration of product species raised to the power of their
According to the Le Chatelier’s principle the change in concentration, volume, pressure, and temperature affect the equilibrium constant of the reaction.
b.
To determine:
The equilibrium expression
Introduction:
The equilibrium constant is a parameter which describes the relationship between the concentration of the reactants and the products at equilibrium stage. The equilibrium constant of a reaction is expressed by the ratio of the concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
According to the Le Chatelier’s principle the change in concentration, volume, pressure, and temperature affect the equilibrium constant of the reaction.
c.
To determine:
The effect of removal of blood glucose on the equilibrium of the given reaction.
Introduction:
The equilibrium constant is a parameter which describes the relationship between the concentration of the reactants and the products at equilibrium stage. The equilibrium constant of a reaction is expressed by the ratio of the concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
According to the Le Chatelier’s principle the change in concentration, volume, pressure, and temperature affect the equilibrium constant of the reaction.
d.
To determine:
The effect of raising the temperature on the equilibrium of the reaction.
Introduction:
The equilibrium constant is a parameter which describes the relationship between the concentration of the reactants and the products at equilibrium stage. The equilibrium constant of a reaction is expressed by the ratio of the concentration of product species raised to the power of their stoichiometric coefficients to the concentration of reactant species raised to the power of their stoichiometric coefficients.
According to the Le Chatelier’s principle the change in concentration, volume, pressure, and temperature affect the equilibrium constant of the reaction.
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Chapter 9 Solutions
GENERAL ORGANIC+BIOL...-MOD.MASTERING..
- a) The F-F bond dissociation energy (BDE) is approximately 37 kcal/mol.For reference, a “normal” C-C or C-H bond has a BDE of approximately 100kcal/mol. Briefly explain why the F-F bond is much weaker than a C-C or C-H bond b) Consider the balanced equation below, where “Ph” indicates amonosubstituted benzene (“phenyl”) ring: Ph-H + F-F -> Ph-F + H-F The BDEs of the molecules involved, in kcal/mol, are as follows:Bond BDE (kcal/mol)Ph-H 112Ph-F 116H-F 136 What is the delta H for the fluorination of benzene by F2? Is the reaction favored or not? c) Why is the fluorination of benzene with F2 rarely done? For reference, thebromination of benzene with Br2 has a delta H of approximately -12 kcal/mol.arrow_forwardConsider the following reaction: H2S (aq) + 2 NaOH (aq) ---> Na2S (aq) + 2 H2O (l). What is located on the product side of this chemical reaction? A. H2S (aq) + 2 NaOH (aq) B. Na2S (aq) + 2 H2O (l)arrow_forwardAre reactants or products favored in the following equation? [Pt(NH3)4]Cl2(aq) + 2 NH2CH2CH2NH2(aq) → [Pt(NH2CH2CH2NH2)2]Cl2(aq) + 4 NH3(aq) Select one: a. products favored, due to the chelate effect b. Cannot determine if products or reactants are favored. c. reactants favored, due to the chelate effectarrow_forward
- Which factor will not increase the concentration of NH3 (ammonia)?N2(g) + H2(g) ⇄ NH3(g) + heatA. Increasing the concentration of H2.B. Increasing the concentration of N2.C. Decreasing the pressure.D. Decreasing the temperaturearrow_forwardThe equilibrium constant for the acid ionization of mercaptoethanol (HSCH2CH2OH) is HSCH2CH2OH(aq) = H+(aq) + SCH2CH2OH-(aq) k= 1.91 x 10-10 Which of the following is/are true regarding this equilibrium? And why? 1. The reaction is product-favored. 2. The reaction is reactant-favored. 3. Equilibrium lies far to the right. 4. Equilibrium lies far to the left.arrow_forwardConsider this equation again: H2CO3 (aq) + H2O (l) double arrows HCO3- (aq) + H3O (aq) Ka of carbonic acid = 4.5 X 10-7 This reaction favors the products This reaction favors the reactants Neither the reactants or products are favored.arrow_forward
- Are reactants or products favored in the following equation? [Pt(NH3)4]Cl2(aq) + 2 NH2CH2CH2NH2(aq) → [Pt(NH2CH2CH2NH2)2]Cl2(aq) + 4 NH3(aq) Select one: a. Cannot determine if products or reactants are favored. b. products favored, due to the chelate effect c. reactants favored, due to the chelate effectarrow_forwardA 0.0670-g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H+ , C2H3O2 - , and HC2H3O2at equilibrium. (Ka for acetic acid =1.76 x 10-5 ).arrow_forwardWhat is the relationship between △G△Go and Keq for the following equilibrium?arrow_forward
- Using the ΔHf values in the appendix, calculate the ΔH of each reaction below. 4 NH3(g) + O2(g) → 2 N2H4(g) + 2 H2O(l)arrow_forwardheat + NH4+ + OH- NH3 + H2O with phenolphalein Pink ⇌ colorless adding NaOH what direction equilibrium is shifted? what happens chemically?arrow_forward1. Henry’s Law constant for most gases decreases with increased temperature. Given that KH for O2 is 2.20 x 10-3 M atm-1 at 5oC, calculate the percent O2(aq) saturation if a lake water sample at 5oC and sea-level is found to contain, 9.20 mg/L of O2(aq). (Recall: partial pressure of O2 at sea-level = 0.2095 atm).arrow_forward
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning