exam 3 ch 17 Flashcards
Which process is spontaneous?
movement of a ball from the bottom to the top of a slide
diffusion of gas from low pressure to high pressure
dissolution of sand in water
saltwater converting into salt crystals and water
evaporation of gasoline
evaporation of gasoline
According to the second law of thermodynamics, the change in the entropy of the universe (ΔSuniv) during a spontaneous reaction is
zero.
negative.
positive.
less than the change in entropy of the system (ΔSsys).
greater than the change in entropy of the system (ΔSsys).
positive.
Which process is nonspontaneous?
Iron in the open air rusts.
Liquid water in a freezer turns to ice.
A spark ignites a mixture of propane and air.
Perfume diffuses in a room.
Heat flows from a cold body to a hot body.
Heat flows from a cold body to a hot body.
In a spontaneous process, which of the following always increases?
the entropy of the system
the entropy of the surroundings
the entropy of the universe
the entropy of the system and the universe
the entropy of the system, the surroundings, and the universe
the entropy of the universe
During a spontaneous chemical reaction, it is found that ΔSsys< 0. This means
ΔSsurr< 0, and its magnitude is less than ΔSsys.
ΔSsurr< 0, and its magnitude is greater than ΔSsys.
ΔSsurr> 0, and its magnitude is less than ΔSsys.
ΔSsurr> 0, and its magnitude is greater than ΔSsys.
ΔSuniv< 0.
ΔSsurr> 0, and its magnitude is greater than ΔSsys.
For a nonspontaneous chemical reaction, it is found that ΔSsys> 0. Which of the following could be true?
ΔSsurr< 0, and its magnitude is less than ΔSsys
ΔSsurr> 0, and its magnitude is less than ΔSsys
ΔSsurr< 0, and its magnitude is greater than ΔSsys
ΔSsurr> 0, and its magnitude is greater than ΔSsys
ΔSuniv> 0
ΔSsurr< 0, and its magnitude is greater than ΔSsys
What is the entropy change to the surroundings when one mole of ice melts in someone’s hand if the hand temperature is 32°C? Assume a final temperature for the water of 0°C. The heat of fusion of ice is 6.01 kJ/mol.
-188 J/K
+19.7 J/K
-22.0 J/K
+188 J/K
-19.7 J/K
-19.7 J/K
If one mole of ice melts at its melting point of 273 K, the entropy change for the ice is 22.0 J/K. If the ice melts in someone’s hand at 34°C, what is the change in the entropy of the universe? Assume a final temperature for the water of 0°C. The enthalpy of fusion for ice is 6.01 kJ/mol.
+19.6 J/K
-2.4 J/K
-19.6 J/K
+41.5 J/K
+2.4 J/K
+2.4 J/K
The entropy change of the surroundings, ΔSsurr, is related to heat transfer, q, with respect to the system and temperature T by
-q/Tsys=ΔSsurr.
+q/Tsys=ΔSsurr.
-q/Tsurr=ΔSsurr.
q/Tsurr=ΔSsurr.
None of these are correct, unless the system undergoes a reversible process.
-q/Tsurr=ΔSsurr.
Care must be taken when dissolving solid pellets of sodium hydroxide (NaOH) in water, because the temperature of the water can rise dramatically. Taking NaOH as the system, what can you deduce about the signs of the entropy change of the system (ΔSsys) and surroundings (ΔSsurr) from this?
ΔSsys< 0 and ΔSsurr< 0
ΔSsys< 0 and ΔSsurr> 0
ΔSsys> 0 and ΔSsurr< 0
ΔSsys> 0 and ΔSsurr> 0
Nothing can be deduced from this limited information.
ΔSsys> 0 and ΔSsurr> 0
The enthalpy of fusion for carbon tetrachloride (CCl4) is 2.67 kJ/mol, and its melting point is 250 K. What is the entropy change when 2.0 mol of carbon tetrachloride melts at 250 K?
21.4 J/K
0.0214 J/K
10.7 J/K
0.0107 J/K
-668 J/K
21.4 J/K
The enthalpy of fusion for benzene (C6H6) is 127.40 kJ/kg, and its melting point is 5.5°C. What is the entropy change when one mole of benzene melts at 5.5°C?
9.95 kJ/K
1.81 J/K
35.7 J/K
127.40 kJ/K
1809 J/K
35.7 J/K
The enthalpy of vaporization for toluene (C7H8) is 380.00 kJ/kg, and its boiling point is 110.6°C. What is the entropy change when 0.75 mol of toluene vaporizes at 110.6°C?
743 J/K
36.3 J/K
139 J/K
253 kJ/K
68.5 J/K
68.5 J/K
The gas above the liquid in a sealed bottle of soda is primarily carbon dioxide. Carbon dioxide is also dissolved in the soda. When the distribution of carbon dioxide between the gas and liquid is at equilibrium, molecules of carbon dioxide in the gas phase can still dissolve in the liquid phase if they strike the surface and are captured. Similarly, molecules of carbon dioxide can escape from the liquid phase. What is the entropy change of the universe, ΔSuniv, for the dissolution of carbon dioxide under these conditions?
ΔSuniv< 0, because the dissolved carbon dioxide has fewer accessible states.
ΔSuniv> 0, because the dissolved carbon dioxide has fewer accessible states.
ΔSuniv= 0, because this is an equilibrium situation.
ΔSuniv< 0, because the gas dissolves spontaneously.
ΔSuniv> 0, because the gas dissolves spontaneously.
ΔSuniv= 0, because this is an equilibrium situation.
Which process will lead to a decrease in the entropy of the system?
Salt crystals dissolve in water.
Air escapes from a hole in a balloon.
Iron and oxygen react to form rust.
Ice melts in your hand.
None of these lead to a negative change in the entropy of the system, because they are all spontaneous.
Iron and oxygen react to form rust.