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Which of the following statements is true?
a) In any spontaneous process, the entropy of the system alwaysincreases.
b) All spontaneous processes are exothermic.
c) Any spontaneous process is accompanied by a positive free energychange.
d) In order for a process to be spontaneous, the process must beexothermic and the entropy of the system must increase.
e) None of the statements above are true.

I know the answer is e, but I don't know why the other answers werefalse and was hoping that someone could shine some light as to whya-d are false. Thanks!

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Reid WolffLv2
29 Sep 2019
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Related questions

Can anyone please explain why ∆S(surroundings) is < 0 ???

What do they mean ∆H (system) > 0? How/why did the system provide heat to dissolve the barium sulfate???

What equation are they drawing from? The only equation I can think of to relate this situation is ∆S(universe) = ∆S(system) + ∆S(surroundings) > 0 (if the process is spontaneous).Does it mean it's not spontaneous if the system provided heat? Maybe this has to do with lattices and hydration - I don't know.

apparently, ∆G for the dissolution of barium sulfate in water is positive.. is dissolution of a sparingly soluble salt always a non-spontaneous process? Thank you!

Please help me - thanks!

1. Check all of the following statements that are true:

a. The value of q is always equal to the value of w for a reversible reaction

b. The energy change of the universe for any spontaneous process is always positive

c. The equilibrium constant is always equal to one for any system at equilibrium

d. The free energy change for any spontaneous process is always positive

e. None of these statements are true

f. The entropy change of the universe for any spontaneous process is always positive

g. The equilibrium constant is always greater than one for an extensive reaction

2. What mass of Na2SO4 is required to make 60 mL of a 0.20 M Na2SO4 solution? Report your answer to three places past the decimal point.

_____g of Na2SO4

3. Select all of the compounds below that are more soluble in water than in CCl4. (You should check anywhere from one to four boxes.)

HCl

NH3

FeCl2

Cl2

None of these are more soluble in water

Model 1 – Spontaneous Processes Process Description Change in Enthalpy (∆H) Change in Entropy (∆S) Spontaneous? A Two pure → Homogeneous substances mixture ~ 0 Increasing Yes B Solute on Solute on one side of → both sides of membrane membrane ~ 0 Increasing Yes C Polypeptide → Individual chain amino acids Exothermic (negative) Increasing (positive) Yes D C3 H8 + 5O2 → 3CO2 + 4H2 O Exothermic Increasing Yes E 6CO2 + 6H2 O → C6 H12O6 + 6O2 Endothermic Decreasing No F Glucose → Starch Endothermic Decreasing No G Water → Ice Exothermic Decreasing Below 0 °C, yes Above 0 °C, no H Cold water (25 °C) → Hot water (60 °C) Endothermic Increasing Below 60 °C, no Above 60 °C, yes

Some of the processes in Model 1 are spontaneous—that is, they will occur without any additional work being done on the system. For example, a solute will diffuse across a membrane until the concentrations of both sides are equal. However, glucose will not spontaneously form from carbon dioxide and water in the atmosphere. The Second Law of Thermodynamics states that a process will be spontaneous when it results in an increase of total entropy in the universe. In other words, either the system or the surroundings must have an increase in entropy, or both. (Please note that the term “spontaneous” does not imply that the change will happen quickly. Rusting is spontaneous under the right conditions, but it can still occur very slowly.)

13. Predict the change in entropy of the surroundings for an endothermic reaction.

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