the pressure exerted by evaporated liquid particles on the surface of the liquid is called:

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