(a)
Interpretation:
The entropy changes in the given processes has to be explained.
Concept Introduction:
In
The SI unit of entropy is J/K.
(b)
Interpretation:
The entropy changes in the given processes has to be explained.
Concept Introduction:
In thermodynamics entropy refers to randomness of the system. Second Law of thermodynamics sates that the entropy of the universe is increasing. That is, the system is always tending to have more disorders in it. Let us consider the example of diffusion of gas molecule to understand the concept of entropy. When a perfume bottle is opened the fragrance is immediately spread into the surroundings. Inside the bottle the gas molecules are close to each other and entropy is less. Once the bottle is opened the gas molecules escapes into the surroundings and have more disorderly arrangements.
The SI unit of entropy is J/K.
(c)
Interpretation:
The entropy changes in the given processes has to be explained.
Concept Introduction:
In thermodynamics entropy refers to randomness of the system. Second Law of thermodynamics sates that the entropy of the universe is increasing. That is, the system is always tending to have more disorders in it. Let us consider the example of diffusion of gas molecule to understand the concept of entropy. When a perfume bottle is opened the fragrance is immediately spread into the surroundings. Inside the bottle the gas molecules are close to each other and entropy is less. Once the bottle is opened the gas molecules escapes into the surroundings and have more disorderly arrangements.
The SI unit of entropy is J/K.
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Chemistry: Atoms First
- a Calculate K1, at 25C for phosphoric acid: H3PO4(aq)H+(aq)+H2PO4(aq) b Which thermodynamic factor is the most significant in accounting for the fact that phosphoric acid is a weak acid? Why ?arrow_forwardWhat is the equilibrium constant expression for the reaction NO2(g) ⇄ N2O4(g)?arrow_forwardWrite the equilibrium-constant expression, Kc, for the following reaction. 3O2(g) ↔ 2O3(g)arrow_forward
- The propionate ion, CH3CH2COO–, reacts with water as a weak base: CH3CH2COO–, (aq) + H2O(l) ⇄ CH3CH2COOH(aq) + OH–(aq), with K = 7.4 x 10-10 at 25°C. If sodium propionate were dissolved in water to make a 0.60 M solution, what would be the resulting concentration of OH–? (no scientific notation)arrow_forwardCalculate the equilibrium constant for the dissociation of dinitrogen tetroxide at 25 °C.2NO2(g) ⇌ N2 O4(g)arrow_forwardWrite the equilibrium-constantexpression and calculate the value of the equilibrium constant and the free-energy change for these reactions at298 K:(a) NaHCO3(s) ⇌ NaOH(s) + CO2(g)(b) 2 HBr(g) + Cl2(g) ⇌ 2 HCl(g) + Br2(g)(c) 2 SO2(g) + O2(g) ⇌ 2 SO3(g)arrow_forward
- Write the equilibrium law expressions that correspond to the following balancedchemical equations:(a) CH3COOH(aq) + MeOH(l) ⇄ CH3COOCH3(aq) + H2O(l)(b) Al2(SO3)3(s) + 6HCl(g) ⇄ 2AlCl3(s) + 3H2O(l) + 3SO2(g) (c) Cu(H2O)4 2+(aq) + 4Cl-(aq) ⇄ CuCl4 2-(aq) + 4H2O(l)arrow_forwardWrite the equilibrium constant expression for each of the following reactions and classify the reactions as homogeneous or heterogeneous. (a) H2S (g) + O2 (g) ↔ H2O (g) + SO2 (g) (b) CO2 (g) + H2 (g) ↔ CO (g) + H2O (l) (c) HCl (g) + O2 (g) + C2H4 (g) ↔ C2H4Cl2 (g) + H2O (g)arrow_forwardCalculate Kp for the following reactions at the indicated temperature. (a) H₂(g) + 1₂(g) 2 HI(g) K = 61.0 at 664 K Кр (b) NH3(g) + HCI(g) ? = NH4CI(S) K = 92.6 at 587 K Кр =arrow_forward
- Write equilibrium constant expression for the following:Fe2O3 (s) + 3 H2 (l) ⇌ 2 Fe (s) + 3 H2O (g)arrow_forwardCaF2(s)⇄Ca2+(aq)+2F−(aq) Ksp=3.9×10−11 HF(aq)⇄H+(aq)+F−(aq) Kc=6.8×10−4 The dissolution of calcium fluoride is represented by the equilibrium system above at 25°C. The F− ion is produced when the weak acid HF dissociates. If solid calcium fluoride is added to equal volumes of the following solutions at 25°C, in which solution will the most calcium fluoride dissolve? a) Pure Water b) 1 M HNO3(aq) c) 1 M NaOH(aq) d) A saturated aqueous CaF2 solutionarrow_forwardAt 25 °C, the following reactions have the equilibrium constants noted to the right of their equations.2CO(g) + O2(g) ⇄ 2CO2(g) Kc= 3.3 × 10912H2(g) + O2(g) ⇄ 2H2O(g) Kc= 9.1 × 1080 Use these data to calculate Kc for the reactionH2O(g) + CO(g) ⇄ CO2(g) + H2(g) Kc = __?arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning