the pressure exerted by evaporated liquid particles on the surface of the liquid is called:
TRANSCRIPT
The pressure exerted by evaporated liquid particles on the
surface of the liquid is called:
• Vapor pressure
Which state of matter has the least attraction between particles?
• gas
• The process in which particles turn from liquid to vapor from the surface of the liquid is called: __________________
• evaporation
• How can a liquid be made to boil below its boiling point?
• Lower the atmospheric pressure
• Two ways that a liquid could be made to boil above its boiling point are:
• Raise the atmospheric pressure
• Add a solute
Which state of matter below has the highest potential energy?
a. Solid b. Liquid c. Gas d. aqueous
C. Gas
• Which state below exhibits the highest entropy?
• a. Solid b. Liquid c. Gas d. aqueous
• C. Gas
• Systems in nature tend to go favor __________ energy and __________ entropy.
• Systems in nature tend to go favor __low________ energy and __high________ entropy
The normal melting point of this substance is approximately:
• 100°C
At 400°C and 1.50atm, this substance is a _________.
• Liquid
The phase change that occurs as the pressure is raised from 0.25atm to 1.25atm at 400°C is called ________. The sign of ΔH
for this phase change is _________;.
• Condensation, negative
The phase change that occurs as the temperature is raised from -100°C to 200°C at 1.25atm is called ________. The sign of ΔH for
this phase change is _________.
• Melting; positive
C2H5OH(l) + 3 O2(g) 2 CO2(g) + 3 H2O (g) ΔH = -1418 kJ
Is energy absorbed or released in the reaction above?
• released
C2H5OH(l) + 3 O2(g) 2 CO2(g) + 3 H2O (g) ΔH = -1418 kJ
• Does entropy increase or decrease in the reaction above?
• What is the sign of ΔS?
• increase
C2H5OH(l) + 3 O2(g) 2 CO2(g) + 3 H2O (g) ΔH = -1418 kJ
• Under what temperature conditions will this reaction be spontaneous?
• Any temperature
• Which sample below has the highest average kinetic energy?– A. Liquid water at 100°C– B. Steam at 100°C– C. Solid lead at 250°C– D. Gaseous nitrogen at 23°C
C. Solid lead at 250°C
• Which sample below has the highest potential energy?– A. Liquid water at 100°C– B. Steam at 100°C– C. Solid lead at 450°C– D. liquid nitrogen at -100°C
• B – steam at 100°C
• Which substance below would have the lowest specific heat capacity?
a. Ironb. SiO2
c. water
• A. Iron
The beaker became warm when the precipitate formed from the supersaturated solution we made.• The sign of ΔH for this process is _________.• The sign of ΔS for this process is ___________.
• ΔH is negative.• ΔS is negative.
m x sh x ΔT = m x sh x ΔT metal water
• While finding the specific heat of a metal in lab, a student takes the initial temperature of the water in the calorimeter without letting the thermometer cool down from measuring the temperature of the metal.
• This would make the calculated specific heat of the metal too _________.
• Too low.
m x sh x ΔT = m x sh x ΔT metal water
• While finding the specific heat of a metal in lab, a student accidentally spilled some of the water from the calorimeter, after he had already recorded its mass.
• This would make the calculated specific heat of the metal too _________.
• Too low
m x sh x ΔT = m x sh x ΔT metal water
• While finding the specific heat of a metal in lab, a student forgets to zero the balance with the cup on it.
• This would make the calculated specific heat of the metal too _________.
• Too high
Which segment(s) on the graph show a change in kinetic energy?
• Segments AB, CD, and EF
The process that occurs moving from point E to point D is called _____________. The sign of ΔH for this
process is _______________.
• Condensation; negative
The melting point of the substance could be determined at points _____ or ______ on the graph
below.
• B or C