Now let's add a third closed container, Sample Z. Sample X: 500 mL of water Sample Y: 1 mole of sugar in 500 mL of water Sample Z: 1 mole of sodium phosphate in 500 mL of water 1. Which sample has the lowest entropy (S)? [Select] 2. Which sample has the lowest free energy (G)? [Select ] 3. Which sample is the most stable? [Select] 4. Which sample has the highest vapor pressure? [Select] 5. Which sample has the highest boiling point? [Select] 6. Which sample has the lowest freezing point? [Select]

Now let's add a third closed container, Sample Z. Sample X: 500 mL of water Sample Y: 1 mole of sugar in 500 mL of water Sample Z: 1 mole of sodium phosphate in 500 mL of water 1. Which sample has the lowest entropy (S)? [Select] 2. Which sample has the lowest free energy (G)? [Select ] 3. Which sample is the most stable? [Select] 4. Which sample has the highest vapor pressure? [Select] 5. Which sample has the highest boiling point? [Select] 6. Which sample has the lowest freezing point? [Select]

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter18: Principles Of Chemical Reactivity: Entropy And Free Energy

Section: Chapter Questions

Problem 2PS: Acetic acid, a weak acid, was added to a beaker containing water at 25 C, giving a solution...

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Acetic acid, a weak acid, was added to a beaker containing water at 25 C, giving a solution containing molecular acetic acid, hydronium ion, and acetate ion at equilibrium. The temperature did not change. (a) Is the solution process exothermic or endothermic? (b) Was the dissolving process and partial ionization spontaneous? (c) Did the entropy of the system increase or decrease? (d) Did the entropy of the universe increase or decrease?
TRUE OR FALSE? 1. Entropy changes cannot be measured with a calorimeter like enthalpy changes. 2. If the result upon calculation of entropy changes in the universe is a positive value, the process is reactant-favored. 3. If the change in free energy, ΔG is negative, the reaction is spontaneous in the forward direction.
choose the right options -When a solid dissolves in a liquid, entropy usually (increases or decreases?) So the value for ΔΔS is (positive or negative?) Remember that negative values of ΔΔG are favorable, and ΔΔG = ΔΔH - TΔΔS. Consequently, solids are usually more soluble at (higher or lower?) temperatures. When a gas dissolves in a liquid, entropy usually (increases or decreases), so the value for ΔΔS is (negative or postive) Remember that negative values of ΔΔG are favorable, and ΔΔG = ΔΔH - TΔΔS. Consequently, gases are usually more soluble at (lower or higher) temperatures.
TRUE OR FALSE? If the system is in order manner, the change in entropy is lower. Which of the following decreases in entrophy? Ice cream melts Water vapor deposits as ice crystals on cold window panel Iodine crystals undergo sublimation Sugar dissolves in a cup of water Water is heated until lukewarm
Calculate ΔHrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔHΔH values: C(s)+2H2(g) →CH4, ΔH=-74.6 kJ C(s)+2Cl2(g) → CCL4(g), ΔH=-95.7 kJ H2(g)+Cl2 → 2HCl (g), ΔH= -184.6 kJ
Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 3 NO(g) → N2O(g) + NO2(g) A) -23.0 kJ B) 69.0 kJ C) -69.0 kJ D) -7.67 kJ E) 23.0 kJ
Evaluate each reaction below and using your knowledge of entropy, predict whether entropy will increase or decrease as reactants are converted to products. Reaction Will entropy increase or decrease? 2 NH3(g) → N2(g) + 3 H2(g) increase or decrease PbS(s) → Pb2+(aq) + S2-(aq) increase or decrease CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) increase or decrease N2(g) + 3 H2 (g) → 2 NH3 (g) increase or decrease
1. What is the Gibbs Free Energy change of a reaction that has Keq of 12.5 at 25degC? a.6.26 kJ/mol b.-6.26 kJ/mol c.6.26 J/mol d.-6.26 J/mol
Which has lower entropy? CO2(g) or CH4(g)?
Predict whether the entropy of the following reaction will increase or decrease. Explain why you would predict this. 2 NH3(g) → N2(g) + 3 H2(g)
Find the ΔH (in kJ) for the reaction: PCl3(l) + Cl2(g) → PCl5(s) Given: 2 P (s) + 3 Cl2(g) → 2 PCl3(l) ΔH = -640 kJ2 P (s) + 5 Cl2(g) → 2 PCl5(s) ΔH = -886 kJ
a) The following reaction occurs in an open beaker: C2H5OH (g) ---> C2H4(g) + H2O (g) {Bond Energy (kJ/mol): C-H = 415 ; C-C = 345 ; C-O = 350 ; O-H = 464 ; C=C = 611}i) Calculate the ΔH0rxn for this reaction from the given bond energies. kJ ii) Is this reaction an open, closed or isolated system? iii) Would you feel hot or cold if you were near this reaction when it occurred? This is because (choose from I - V) I. the reaction is exothermic and absorbs energy from the surroundings. II. the reaction is exothemic and releases energy to the surroundings. III. the reaction is endothermic and absorbs thermal energy from the surroundings. IV. the reaction is endothermic and loses heat to the surroundings. V. the reaction produces steam which contains a lot of heat.