Concept explainers
- a)
Interpretation:
The reaction which give larger
Concept Introduction:
Equilibrium constant: The equilibrium constant of a
Gibb’s free energy: The Gibb’s free energy also termed as the available energy; is the
To Identify: The reaction which give larger
- b)
Interpretation:
The reaction which give larger
Concept Introduction:
Equilibrium constant: The equilibrium constant of a chemical reaction is the value of its reaction quotient at chemical equilibrium.
Gibb’s free energy: The Gibb’s free energy also termed as the available energy; is the thermodynamic potential that is minimized when a system reaches chemical equilibrium at constant and temperature.
To calculate equilibrium constant
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Chemistry
- Consider the following equation: [Ni(H2O)6]2+ + 6NH3 <----> [Ni(NH3)6]2+ +6H2O The effects of stress on this equilibrium can be monitored by changes in color. An equilibrium mixture is blue-green (indicating both products and reactants are present). a.) When the equilibrium mixture is heated, the color changes to bright green. Which direction has the reaction shifted? To the products, the reactants, or no shift? How did you determine this? Which is the exothermic direction of this reaction? Forward, reverse, or cannot tell? b.) When a few drops of concentrated NH3 are added to the equilibrium mixture, the solution turns deep blue. Which direction has the reaction shifted? To the products, the reactants, or no shift? How did you determine this? c.) Addition of concentrated HNO3 to the blue-green mixture will remove NH3 by reaction. What should happen to the color of the solution? Will it turn more blue, turn more green, or no change? Explain.arrow_forwardFor each of the following reactions, identify the acid and the base. Also indicate which acid-base definition is most applicable. Fe3+ + 6 SCN– →[Fe(SCN)6]3– HClO4 + (CH3)3N → (CH3)3NH+ + ClO4– [Co(H2O)6]2+ + 4 HCl → [CoCl4]2– + 4 H3O+ + 2 H2Oarrow_forwardWhich of the following compounds can exhibit cis-trans isomerism? [Co(H2O)4Cl2]+ [Co(H2O)5Cl]2+ [Co(NH3)6]3+ [Co(H2O)3Cl3]arrow_forward
- During the formation of a coordination compound, the metal acts as a Arrhenius acid Bronsted-Lowry base Lewis base Lewis acid Bronsted-Lowry acidarrow_forwardUsing Le Chateliers Principle, aan you help me understand what are the net ionic equations for the reactions below? the overall reaction is: [CoCl4]2– (alc) + 6 H2O (l) ⇌ [Co(H2O)6]2+ (aq) + 4 Cl¯ (aq) Note: ‘alc’ means an alcoholic solution. The ion, [CoCl4]2– (alc), is blue in color and [Co(H2O)6]2+ (aq) is pink. We have a well filled with add 0.10M CoCl2 and add some deioinized water with stirring until a color change from blue to pink (to products). Next, we add a few drops of concentrated HCl and found color change to blue (to reactants).arrow_forwardWhen orange solution containing Cr2O72–ion is treated with an alkali, a yellow solution is formed and when H+ions are added to yellow solution, an orange solution is obtained. Explain why does this happen?arrow_forward
- 6. Ammonia, NH3, is a stronger ligand than Cl- but weaker than CN. Complete the balanced equations for the reactions that are predicted to occur. CoCl(aq) + CN- (aq) → Co(NH3)³+ (aq) + Cl(aq) → Co(CN)6³(aq) + NH3(aq) →→→arrow_forwardOne of the steps for refining silver involves converting silver into dicyanoargenate(I) ions: 4Ag(s) + 8CN−(aq) + O2(g) + 2H2O(l) ⟶ 4[Ag(CN)2]−(aq) + 4OH−(aq)Explain why oxygen must be present to carry out the reaction. Why does the reaction not occur as: 4Ag(s) + 8CN−(aq) ⟶ 4[Ag(CN)2−(aq)?arrow_forwardGiven the following ionization constant values, which is the strongest weak acid? [Co(OH2)61²+: Ka= 5.0 x 10-10 [Fe(OH2)6]2+: K₂= 3.0 x 10-10 [Fe(OH₂)6]³+: K₂= 4.0 x 10-3 [Be(OH2)4]2+: K₂= 1.0 x 10-5 [Cu(OH2)4]2+: Ka= 1.0 x 10-8arrow_forward
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning