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

C 2 H 5 OH (l) + 3 O 2(g)  2 CO 2(g) + 3 H 2 O (g) ΔH = kJ Is energy absorbed or released in the reaction above?

released

C 2 H 5 OH (l) + 3 O 2(g)  2 CO 2(g) + 3 H 2 O (g) ΔH = kJ Does entropy increase or decrease in the reaction above? What is the sign of ΔS?

increase

C 2 H 5 OH (l) + 3 O 2(g)  2 CO 2(g) + 3 H 2 O (g) ΔH = 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. Iron b. SiO 2 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