Consider the process of a nonpolar molecule reversibly entering an aqueous solution: nonpolar molecule(liq) nonpolar solute(aq) In this process, water molecules must form a "hole" in which the nonpolar molecule will reside. This causes the water molecules to form a relatively fixed cage around the nonpolar molecule. For this process, the sign of ASgys is the sign of ASgurr is and the sign of ASUniv is (The surroundings are the Universe minus the contents of the system. Here, the system is the nonpolar molecule plus the water of the solution.)

Consider the process of a nonpolar molecule reversibly entering an aqueous solution: nonpolar molecule(liq) nonpolar solute(aq) In this process, water molecules must form a "hole" in which the nonpolar molecule will reside. This causes the water molecules to form a relatively fixed cage around the nonpolar molecule. For this process, the sign of ASgys is the sign of ASgurr is and the sign of ASUniv is (The surroundings are the Universe minus the contents of the system. Here, the system is the nonpolar molecule plus the water of the solution.)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

2. According to Le Chatelier's principle, it indicates where the balance is favored (Reactants or products) of the following unbalanced reaction H₂O(a) + Fe(s) + H₂(g) + Fe3O4(s) + Heat Write your answer on the line a) Decreases ia [H2): b) The temperature of the system decreases: c) The system pressure increases:
Km.201.
Initially 10.0 mol of ammonia gas is injected into a 4.0 L container. At equilibrium 1.2 mol of nitrogen gas is found in the container. The number of moles of ammonia gas at equilibrium would be? 2NH3(g) + 94 kJ <=====> N2(g) + 3H2(g)
Methane and water react at 600. K according to the equation below. CH4(g) + H2O(g)→ COg) + 3 H2g) AH=205.9 kJ/mol a. Determine the equilibrium constant for the reaction at 600. K. b. A reaction vessel containing CH4, CO and H2O is heated to 600 K where the pressures are 16.8 atm CH4, 2.97 atm CO and 0.0103 atm H2O. Determine the equilibrium pressure of hydrogen.
Draw the organDraw the organic molecule(s) which is (are) formed in the following reaction. Do not include molecules like H2O or HCI. ic
For the equation: CH3OH (l) + 3/2 O2(g) -> CO2 (g) +2H2O What drives this reaction to go in the forward direction? Entropy, Enthropy, both, or neither?
26) Suppose that at a pressure of 1 atm and temperature 300 K, a given material has two possible phases: liquid (L) and solid (S). We start the system with N₁ = 5 moles in the liquid phase and Ng = 9 moles in the solid phase. For these values of pressure and temperature, PL = 5 x 10-21 J • Hs9 x 10-21 J. What is the equilibrium value of NL? a. 9 mol b. 14 mol c. 1.49 mol d. 5 mol e. O mol
Consider the reaction: PbCl2(s) → Pb2*(aq) + 2 Cl (aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PbCl2 is dissolved in water at 25°C, what are the concentrations of Pb2* and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+: mol/L and Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 10-3 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-³M is kJ/mol. Show your calculations on the separate sheet of paper.
Water freezes spontaneously at -5°C and 1atm. Describe how a spontaneous process can result in a decrease in entropy.